AFNS Most Repeated Chemistry MCQs
| Question | Answer |
| Which of the following sulphur compounds shows +4 oxidation state? | H₂SO₃ |
| Low CO₂ favors stomata to? | Open |
| Ripening of fruits is hastened by which gas? | Ethylene |
| The natural rubber is a polymer of? | Isoprene |
| Seventh period consists of normal elements? | No |
| Halogens exist in which states? | All |
| Two ice cubes are pressed over each other and unite to form one cube. Which force is responsible for holding them together? | H-Bonding |
| The reaction of sodium acetate with soda lime gives? | Methane |
| Picric acid is formed when which compound reacts with nitric acid? | Phenol |
| X-rays are produced when a stream of electrons in an X-ray tube? | Strikes the metal target |
| The reaction in which energy is evolved is called? | Exothermic |
| Which is a buffer solution? | Blood |
| Lead contains? | Sulphuric acid |
| How many molecules are there in one mole of H₂O? | 6.02 × 10²³ |
| Numerical value of Avogadro’s number? | 6.02 × 10²³ |
| Heating of food in a microwave oven is an example of? | Solvent extraction |
| Main component of an organic compound? | Carbon |
| The main source of organic compounds? | Petroleum (if missing: Coal, if both missing: Coal tar) |
| The reactant which is consumed earlier is called? | Limiting Reactant |
| Neutron is discovered by? | Chadwick |
| Which one is not a base? | BF₃ |
| Lattice energy is also called? | Lattice enthalpy |
| If Nitrous oxide gas is inhaled, it causes? | Laughter/Laughing |
| Ionic bond is formed by? | Positive and Negative ions |
| Color of chlorine gas? | Yellow-Green |
| Which series includes the Hydrogen Atom? | Balmer Series |
| Which scientist played an important role in the periodic table? | Mendeleev |
| 760 torr is equal to how many atm/Pascal? | 1 atm / 101325 Pascal |
| Nature of bonds in diamond? | Covalent |
| How many types of intermolecular forces are there? | 3 |
| When compressed Acetylene/Hydrogen is allowed to expand, it causes? | Frostbite |
| Question | Answer |
| What is the boiling point of water at Mount Everest? | 70°C |
| Ethyl acetate is the ester of ethanol and? | Acetic acid |
| Which one halogen is a? | Bromine |
| What is the percentage of sodium in NaOH? | 57.48% sodium, 40% oxygen, 2.52% hydrogen |
| Molarity of HCl is? | 12.1 M (Molar) |
| Molarity of ammonium hydroxide (NH₄OH) is? | 14.5 M |
| Glucose reacts with bromine water to produce? | Gluconic acid |
| Total number of d-block elements in the periodic table? | 40 |
| Ionic bond is formed by? | Positive and Negative ions |
| Reacting bromine with benzene in the presence of sunlight results in? | Addition Reaction |
| Ammonium Chloride is in nature. | Acidic |
| Alcohol reacts with carboxylic acid in the presence of? | H₂SO₄ |
| Acyl Chloride is formed when carboxylic acid reacts with? | Thionyl Chloride (SOCl₂) |
| In an exothermic reaction, heat is? | Released |
| Which gas diffuses more rapidly, H₂ or N₂? | H₂ |
| Heterogeneous mixtures can be separated by? | Distillation/Filtration |
| Alkali is a ? | Base |
| Effusion and Diffusion Process are completely understood by? | Graham’s Law |
| Spontaneous reaction is? | Exothermic |
| Down’s cell is used to prepare? | Sodium Metal |
| A law in which temperature is kept constant is called? | Boyle’s Law |
| Water is sparingly soluble in? | Ethane |
| Dalton’s Law is about? | Atmospheric Pressure |
| Percentage of carbon dioxide carried in the form of bicarbonate in plasma is? | 70% |
| One or two species having the same atomic number and the same position in the periodic table are called? | Isotopes |
| The Laughing Gas is? | N₂O |
| In the periodic table, elements having different properties are? | Lithium and Barium |
| Elements that have more than one form are called? | Allotropes |
| Empirical Formula of Water is? | H₂O |
| In gases, when temperature increases, viscosity of gases? | Increases |
| Which scientist played an important role in the periodic table? | Dimitri Mendeleev |
| Elements at the same position in the Periodic Table are? | Isotopes |
| Covalent Bond is not found in? | Iron |
| Elements that have the same atomic number but different atomic masses are called? | Isotopes |
| Which of the following are diagonal to each other? | Lithium and Barium |
| Question | Answer |
| Which one is not a base? | Hydrochloric acid |
| Lead contain; | Hydrochloric acid |
| In which law, the pressure is kept constant? | Charles’s Law |
| Color of chlorine is; | Yellow-green |
| Who discovered neutron and when? | Chadwick in 1932 |
| Numerical value of Avogadro’s number; | 6.02 x 10²³ |
| How many molecules are there in one mole of H₂O? | 6.02 x 10²³ |
| 760 torr are equal to how many pascal? | 101325 |
| The reactant which is consumed earlier and gives least quantity of product is called; | Limiting reactant |
| When compressed hydrogen is allowed to expand rapidly, it causes; | Respiratory disease |
| Which scientist played a role in the periodic table? | Dimitri Mendeleev |
| How many types of intermolecular forces are there? | 3 |
| The nature of the bond in diamond is; | Covalent |
| Lattice energy is also called as; | Lattice enthalpy |
| Inhaling Nitrogen oxide causes; | Laughter |
| The main source of organic compound is; | Coal |
| A law in which pressure of a given mass of an ideal gas is inversely proportional to its volume at a constant temperature is called; | Boyle’s Law |
| Water is sparingly soluble in; | Ethane |
| Down’s cell is used to prepare; | Sodium metal |
| Effusion and diffusion processes were completely understood by; | Graham’s Law |
| Alkali is a; | Base |
| Which of the following gases diffuse rapidly? | Oxygen |
| Which product is formed when Acyl chloride combines with carboxylic acid? | Acetic anhydride |
| What will be the effect on the rate of reaction when the temperature increases? | Rate of reaction increases |
| What will be the energy on the product side, when an exothermic reaction occurs? | Energy decreases |
| Mass of sulfur in 24.5g of H₂SO₄; | 8g of sulfur |
| 1 Calorie = ? | 4184 Joule |
| Which has the maximum “n” shell electrons? | n=16 |
| The stability of an atom is directly proportional to; | Isotopes |
| What is ethyl acetate? | An organic compound (C₄H₈O₂) used in nail polish remover |
| When Carboxylic acid and Alcohol combine and form an ester, which catalyst is used? | Sulfuric acid (H₂SO₄) |
| Which one of the halogens is liquid? | Bromine |
| Total number of d-block elements in the periodic table; | 30 |
| There are——— Groups in the periodic table; | 18 |
| Two or more forms of an element that contain equal numbers of protons but different numbers of neutrons in their nucleus are called; | Isotopes |
| What is the name of the process in which oxygen is removed? | Reduction |
| Which one is alkaline among the following? | Ammonia |
| Which acid is used in the body to help digestion? | Boric acid |
| CNG stands for; | Compressed Natural Gas |
| Picric acid is formed when———– reacts with nitric acid. | Phenol |
| Down’s cell is used to prepare; | Sodium metal |
| Dalton’s Law is about; | Partial Pressure |
| A heterogeneous mixture can be separated by? | Distillation / Filtration |
| What law is when pressure is inversely proportional to volume? | Boyle’s Law |
| What law is when the pressure is constant? | Charles’s Law |
| Melting point of NaCl is? | 801°C |
| Calcium Carbide on reaction with water gives; | Acetylene gas and calcium hydroxide |
| The shape of an orbital is determined by which quantum number? | Azimuthal Quantum Number |
| Size and energy of an orbital are determined by? | Principal Quantum Number |
| What is the boiling point of water at Murree? | 98°C |
| Question | Answer |
| The covalent radius of Cl atom is: | 99 pm |
| CsF is an ionic compound because: | Low IP of Cs and high EA of F |
| Molecular orbitals are filled with the available electrons according to: | Hund’s rule |
| An ionic compound will dissolve in water only if: | Hydration energy is high and lattice energy is low |
| A chemical bond between two atoms having the difference of electronegativity 1.7 then which statement is correct: | Bond is 50% ionic and 50% covalent |
| Which of the following compound has ionic bond in it: | NaF |
| Which of the following is most electronegative element: | F |
| The energy that is required to remove an electron from an atom is called: | Ionization potential |
| The tendency of bonded atom in a molecule to attract shared pair of electrons is called: | Electronegativity |
| Which of the following element has highest ionization potential: | Rb |
| In a group of periodic table, ionization energy: | Decreases |
| The strongest bond is: | C≡C |
| Which of the following is not correct: | Single bond is shorter than double bond |
| In which of the following pairs, do the elements form a compound by sharing electrons: | Carbon and chlorine |
| Molecular orbital theory explains well: | All of above |
| The expected geometrical shape of molecules which have sp³ hybridization is: | Pyramidal |
| Which of the following compounds have ionic, covalent and coordinate bond in it: | HNO3 |
| Which of the following species has highest bond order: | O₂⁺ |
| The study of heat changes accompanying a chemical reaction is known as: | Thermochemistry |
| If an endothermic reaction is allowed to take place very rapidly in air, the temperature of the surrounding air: | Decreases |
| In endothermic reactions, the heat contents of the: | Products more than that of reactants |
| The majority of reactions which give stable products are: | Exothermic |
| It is noticed that energy in the form of heat is either evolved or absorbed as a result of a: | Chemical change |
| In a chemical change, the energy in the form of heat will either be evolved or absorbed and this is called: | Heat of reaction |
| The energy units in which heat changes usually expressed in SI-system are: | Joule |
| The subject matter of first law of thermochemistry is based on: | First law of Thermodynamics |
| A process which takes place on its own from a non- equilibrium state towards an equilibrium state is termed as: | Both Spontaneous and Natural process |
| Which one of the following is not related to spontaneous process: | Artificial |
| Neutralization of a strong acid with a strong base is: | Both Natural acid base reaction and Spontaneous acid base reaction |
| When a piece of zinc is added to the copper sulphate solution, colour of solution disappear: | Blue |
| The reaction of Zinc with copper sulphate solution is an example of: | Spontaneous redox reaction |
| A reaction will also be called a spontaneous if: | It does not need energy to start with |
| Burning of coal and hydrocarbon in air are examples of: | Both Spontaneous reaction and Natural reaction |
| Some non-spontaneous processes can be made to take place by supplying energy to the system from: | All of above |
| By state, we mean the: | Condition of a system |
| When no work is done by the system: | The volume of system decreases |
| Question | Answer |
| The experimental evidences for the existence of atomic nucleus comes from: | Scattering of alpha particles by thin metal foil |
| When alpha particles are bombarded over Be atoms, neutrons are released along with: | Carbon |
| The Rutherford experiment of using a stream of alpha particles on a piece of gold foil proved that: | Atom had a great empty space in it |
| Which of the following observations was seen by Rutherford when alpha particles were bombarded over gold | Majority of alpha particles passed through foil without deflection |
| foil? | |
| The mass of alpha particle is equal to: | Four times the mass of one proton |
| Rutherford’s model of atoms failed because: | It did not account for stability of the atom |
| Max Planck proposed quantum theory in: | 1900 |
| Quantum theory explained: | Both emission and absorption of radiations |
| According to Planck energy travels in a discontinuous manner and it is composed of large number of tiny discrete units called: | Quanta |
| The value of Planck’s constant ‘h’ is: | 6.625 x 10^-34 Joule second |
| According to Planck, in case of light, the quantum of energy is often called: | Photon |
| Wavelength is the distance between two adjacent crests or troughs and expressed in: | nm |
| Greater the wavelength associated with the photon: | Smaller is its energy |
| Energy of a photon is related to: | All of above |
| Greater the wave number of photons: | Greater is the energy associated with them |
| Splitting of spectral lines when atoms are subjected to a strong electric field is called: | Stark’s effect |
| The velocity of photon is: | Independent of its wavelength |
| Bohr’s model of atom explains spectrum of: | H atom only |
| Transition from various energy levels to the lowest energy level gives: | Lyman series |
| P-fund, Bracket and Paschen series lie in: | Infrared region |
| Balmer series lie in: | Visible region |
| The force which holds together two or more atoms or ions to form a large variety of compounds is called: | A chemical bond |
| The theory of chemical bonding has been a major problem of: | Modern Chemistry |
| Chemical reactivity of elements depends upon their characteristic: | Electronic configurations |
| Which of the following elements is not stable: | Kr |
| Elements combine together due to inherent tendency to stabilize themselves by: | Losing electron, Sharing electrons, Gaining electrons |
| Which of the following is a noble gas: | Ne |
| The tendency of atoms to attain a maximum of eight electrons in the valence shell is known as: | Octet rule |
| In the chemical combination of sodium and hydrogen to form NaH: | Hydrogen atom gains an electron |
| In the chemical combination of hydrogen and fluorine to form HF: | Both atoms share the electrons equally |
| Which of the following molecules is not formed according to octet rule: | XeO3 |
| According to modern theory of chemical bonding, atoms form bonds as it leads to a: | Decrease in energy |
| When two hydrogen atoms approach each other: | Forces of attraction and repulsion operate simultaneously |
| The bond length between atoms of hydrogen in the hydrogen molecules is: | 0.0754 nm |
| Which of the following has smaller size: | Fe³⁺ |
| In a group of periodic table, atomic radii: | Increases |
| In a period of periodic table, atomic radii: | Decreases |
| Which statement is true for Na and Na⁺: | Size of Na is greater than Na⁺ |
| As the nuclear charge increases, the pull on the electrons is increased and size of an atom: | Decreases |
| The radius of the ion while considering it to be spherical in shape is called: | Ionic radii |
| The decrease in radius is larger for: | Trivalent ions |
| The increase in size of the anion is due to: | Increase in electron-electron repulsion |
| Question | Answer |
| 8. Rate of evaporation and rate of condensation at equilibrium: | Become equal |
| 19. At sea level and at 100°C the vapour pressure of | 760 mm Hg |
| water in an open system is: | |
| 20. A liquid on evaporation causes: | Cooling effect |
| 21. Escape of high energy molecules from the surface of a liquid is called: | Evaporation |
| 22. Which of the following liquids has low vapour pressure at 25°C: | Water |
| 23. The boiling point of NH3 is maximum among the hydrides of group V elements due to: | Enhanced electronegative character of Nitrogen |
| 24. Heat of vapourization for liquids with strong dipole- dipole forces will have: | Very high values |
| 25. Trend of boiling point of halogens from fluorine to iodine is that it: | Increases |
| 26. Liquids have low boiling point provided: | High vapour pressure at given temperature |
| 27. Molar heat of vapourization of water is: | 40.6 KJ/mole |
| 28. Boiling point for water under 23.7 torr external pressure is: | 25°C |
| 29. Boiling point of a liquid at high altitudes: | Lower at high altitude |
| 30. Cooking time reduces in a pressure cooker because: | Boiling point of water increases |
| 32. Boiling Point of a liquid is high when: | Hydrogen bonding is present |
| 33. Boiling point of a liquid depends upon: | External pressure |
| 34. In the industrial purification of glycerine, its boiling point is reduced from 290°C to 120°C by: | Decreasing external pressure |
| 35. Many organic compounds and biological tissues behave as: | Liquid crystals |
| 36. Which is not the use of liquid crystals? | Energy supply in electrical devices |
| 37. Oscillographic and TV displays also use: | Liquid crystal screens |
| 38. Amorphous solids are characterized by: | Possessing irregular arrangement of atoms |
| 39. Which one of the following is pseudosolid? | Glass |
| 40. Hydrocarbons which generally have high molecular masses, exist in: | Solid form |
| 1. Neutron was discovered by: | Chadwick |
| 2. The e/m value for positive rays is maximum for: | Hydrogen |
| 3. The nature of positive rays depend on: | All of the above |
| 4. Which of the following was discovered first? | Charge of electron |
| 5. Which of the following particles has longest wavelength, if they have same speed? | Electron |
| 6. Maximum potential energy that an electron can have within the atom is: | Infinite |
| 7. Charge to mass ratio of electron was discovered by: | J.J. Thomson |
| 8. When an electric current is passed through discharge tube at low pressure, cathode rays are emitted from cathode these rays consist of: | Negative particles |
| 10. Charge of an electron is: | 1.6 x 10^-19 C |
| 11. Mass of simple electron is: | 9.1 x 10^-31 kg |
| 12. The charge over mass ratio of electron is: | 1.7588 x 10^11 C/Kg |
| 13. Charge on electron was discovered by: | Millikan |
| 14. Proton was discovered by: | Goldstein |
| 15. Which one of the following particles has a mass 1/1836 time, that of hydrogen? | Electron |
| 16. Negatively charged particle nature of cathode rays was first demonstrated in 1895 by: | Hittorf |
| 17. With the reference of e/m ratio of anode rays, the e/m ratio of cathode rays is: | Greater |
| 18. Which one of the following statements is true about discovery of neutrons? | These particles were formed by the bombardment of α-particles on Beryllium |
| 19. Anode is the surface on which probability of finding electron is: | Less than 10% |
| Question | Answer |
| 23. The product of pressure and volume remains constant when temperature and quantity of gas is: | Kept constant |
| 24. The ratio of volume to temperature on Kelvin scale is constant according to: | Charles’s law |
| 25. The graph between pressure and volume at constant temperature for a gas is: | Isotherm |
| 26. The density of a gas is directly proportional to pressure, inversely proportional to temperature, and directly proportional to: | Momentum |
| 27. If absolute temperature of a gas is doubled and the pressure is reduced to one half, the volume of the gas will be: | Increased four times |
| 28. Absolute temperature of a gas is proportional to: | Translational Kinetic energy |
| 29. The highest temperature at which a substance can exist as a liquid is called its: | Critical temperature |
| 30. Keeping the temperature constant, if the gas is expanded: | Pressure will decrease |
| 31. At constant temperature, when pressure of a gas is plotted against volume, the curve is: | Parabolic |
| 32. A gas is heated in such a way that its volume and absolute temperature both are doubled. The pressure of the gas: | Becomes half |
| 33. If the number of gas molecules is doubled in a certain volume, the pressure is: | Increased to half |
| 34. At the same temperature, which substance has high kinetic energy: | Solution of alcohol and water |
| 35. Which one of the following gases has the lowest density at room temperature? | H2 |
| 36. Which one of the following values of the R constant is not correct? | 1.987 cal K^-1 mol^-1 |
| 37. Which of the following equations is for real gas? | PV = nRT |
| 38. If T, M, V, and P are gas constant temperature, molar mass, volume, and pressure, then density is given by: | PM/RT |
| 39. General gas equation can be derived by combining: | Boyle’s law, Charles’s law, and Avogadro’s law |
| 40. The value of general gas constant R is derived from: | Avogadro’s, Coming, and Maxwell’s law |
| Question | Answer |
| 24. Naphthalene, iodine, and NH4 can: | Sublime |
| 26. In a better method, the process of sublimation is carried out in a: | Cold finger |
| 27. Which of the following substances is not a sublime material? | Potash alum |
| 28. Which of the following methods is used to obtain iodine present in the water? | Sublimation |
| 29. Solvent extraction method is a particularly useful technique for separation when the product to be separated is: | Volatile and thermally unstable |
| 30. Solvent extraction is an unstable process and it is controlled by: | Distribution law |
| 31. The most common laboratory example of solvent extraction is: | Ether extraction |
| 32. The other name for distribution law is: | Partition law |
| 33. In CCl4 solvent, I2 shows: | Purple colour |
| 34. The comparative rates at which solutes move in paper chromatography depend on: | Rf value of the solute |
| 35. To help diagnose illness, doctors often need to know which amino acids are present in urine or blood, which method is commonly called: | Chromatography |
| 36. The components of which mixture can be separated by chromatography? | Blue and red inks |
| 37. In chromatography, the point at which solvent maximum rises is called: | Solvent front |
| 38. Chromatography involves the distribution of a solute between: | A stationary and a mobile phase |
| 39. Chromatography in which stationary phase is a liquid is called: | Partition chromatography |
| 40. Chromatography in which stationary phase is a solid is called: | Adsorption chromatography |
| 1. Which of the following is the simplest form of matter? | Gaseous state |
| 2. The movement of gas molecules from a region of high pressure to vacuum is called: | Diffusion |
| 3. All gases can be compressed by: | Increasing pressure |
| 4. Gases exert pressure on walls of the container because the gas molecules: | Collide with the walls of the container |
| 5. Gases of air always remain in random motion and do not settle due to: | Elastic collision of gas molecules |
| 6. The rate of diffusion of a gas is: | Inversely proportional to square root of its molecular mass |
| 7. In gases and liquids, temperature is the measure of: | Average translational kinetic energies of molecules |
| 8. In solids, the temperature is the measure of: | Vibrational kinetic energies |
| 9. Cooling happens under the Joule Thomson effect due to sudden: | All of the above |
| 10. They spread throughout the vessel: | Pressure is due to collision |
| 11. Pressure is due to: | Internal and external conditions |
| 12. Liquids are less common than: | Gases |
| 13. The intramolecular forces in gases are: | Very weak |
| 14. The relationships between volume of a given amount of gas and the prevailing conditions of temperature and pressure are: | Gas laws |
| 15. In Boyle’s law, which of the following pair remains constant: | Temperature and quantity of a gas |
| 16. In Boyle’s law, which of the following pair is variable: | Pressure and Volume |
| 17. For a gas obeying Boyle’s law, if pressure is doubled, the volume becomes: | One half |
| 18. Boyle’s law is represented as: | PV = k |
| 19. According to Boyle’s law, which parameters give a straight line parallel to the x-axis, when we plot a graph between: | P and 1/V |
| 20. Boyle’s law does not fail even: | Pressure is extremely high |
| 21. A graph between P and 1/V at constant temperature and number of moles of a gas meets the: | y-axis |
| 22. A graph between P and PV at constant temperature and number of moles is parallel to: | x-axis |
| Question | Answer |
| Which of the following is NOT an alcohol? | CH3-O-CH3 |
| Fossil fuels consist of: | All of these |
| Geological survey of Pakistan estimates about billion tons of coal in Pakistan: | 184 |
| Major component of natural gas is: | Methane |
| At present oil refineries in Pakistan are: | Four |
| Cracking products are: | Alkanes and alkenes |
| Types of cracking are: | All a, b, c |
| Tetraethyl lead causes disease: | Respiratory |
| The general formula of saturated alicyclic hydrocarbons is: | CnH2n |
| Diversity of organic compounds in millions is: | Six |
| General formula of carboxylic acids is: | RCOOH |
| Linear geometry is present in: | sp |
| Angle 120° is observed in molecules: | CH2=CH2 |
| Preparation of vegetable ghee involves: | Hydrogenation |
| Formula of chloroform is: | CHCl3 |
| The presence of a double bond in a compound is the sign of: | Unsaturation |
| Vinyl acetylene combines with HCl to form: | Chloroprene |
| The addition of an unsymmetrical reagent to an unsymmetrical alkene is in accordance with the rule: | Markownikoff’s rule |
| Synthetic rubber is made by polymerization of: | Butene |
| β,β’-dichloroethyl sulphide is commonly known as: | Mustard gas |
| When methane reacts with Cl2 in the presence of diffused light, the products obtained are? | Mixture of a, b, c |
| Which one of the following gases is used for artificial ripening of fruits? | Ethyne |
| Reaction of ethenes with KMnO4 gives: | Hydroxylation |
| The branch of science dealing with structure, composition, and changes in matter and laws and principles which govern these changes is called: | Chemistry |
| Smallest particle of an element which may or may not have independent existence is known as: | Atom |
| Matter is defined as anything which occupies space and: | Mass |
| The number of atoms present in a molecule determines its: | Atomicity |
| When an electron is added to a unipositive ion, we get: | Neutral atom |
| CO is an example of: | Stable molecule |
| The diameter of atoms is of the order: | 2 x 10^-10 m |
| Swedish chemist J. Berzelius determined: | Atomic mass |
| Covalent compounds mostly exist in the form of: | Molecules |
| Atoms and molecules can either gain or lose electrons, forming charged particles called: | Ions |
| Metals tend to lose electrons, becoming: | Positively charged ions |
| Non-metals tend to gain electrons, becoming: | Negatively charged ions |
| First atomic theory was put forward by an English school teacher: | John Dalton |
| Determination of atomic masses and invention of system of writing symbols was made by: | J. Berzelius |
| Atoms can be evident by the use of electron microscope, field ionization microscope and: | X-rays |
| The number of subatomic particles in atoms so far discovered is more than: | 110 |
| C6H12O6 and C11H22O11 are: | Poly-atomic molecules |
| Cl2, N2 and O2 are: | Diatomic molecules |
| He, Ar and Ne are: | Mono-atomic molecules |
| NH3, HCl, H2O, HI are: | Hetero-atomic molecules |
| Haemoglobin contains nearly: | 10,000 atoms |
| Haemoglobin is 63,000 times heavier than: | Hydrogen atom |
| Molecules of high molecular weight usually greater than 10,000 are called: | Macromolecules |
| Which statement about an atom is true? | Mass number can be equal to the atomic number |
| Which statement about a molecule is incorrect? | Haemoglobin is a homo- atomic molecule |
| A species having positive or negative charge is called: | Ion |
| An ion bearing positive charge is called: | Cation |
| An ion having negative charge is called: | Anion |
| Formation of a cation is: | Exothermic process |
| Anions are larger than their: | Parent atoms |
| Any molecular species having positive charge is called: | Molecular ion |
| Molecular ions are formed in an instrument called: | Mass spectrometer |
| The mass of a molecular ion can be calculated from its: | m/e ratio |
| The mass of one atom of an element compared with the mass of an atom of carbon taken as 12 is called: | Relative atomic mass |
| Due to stability and abundance of carbon compounds, carbon is taken as: | Standard |
| The masses of the atoms are extremely: | Large |
| Relative atomic mass of O is: | 15.9994 amu |
| Isotopes are sister atoms of the same element with similar chemical properties but different: | Atomic mass |
| Isotopes of an element are recorded separately in: | Mass spectrometer |
| Analytical chemistry is the science of: | Chemical characterization |
| A complete chemical characterization of a compound must include: | Both (Qualitative analysis and Quantitative analysis) |
| Estimation of Na in sea water is an example of: | Quantitative analysis |
| Identification of a substance, determination of its structure, and quantitative analysis of its composition are the aspects covered by: | Modern analytical chemistry |
| The detection of a functional group is called: | Qualitative analysis |
| The sample being analyzed is called: | Analyte |
| The solid remained on filter paper during filtration is called the: | Residue |
| The filtration process is used to separate solid from: | Liquid |
| The tip of the funnel should be 1 or 2 cm larger than the circle of the: | Filter paper |
| The tip of the funnel should touch the side of the beaker in order to avoid: | Splashing |
| Selection of filter paper depends upon sizes: | All of the above |
| The liquid obtained after passing the mixture through filter paper is formed as: | Filtrate |
| The apex angle of the folded filter paper is slightly greater than: | 60° |
| Without proper suction, filtration is: | Slow process |
| Fluted filter paper is used to: | Increase rate of filtration |
| Gooch crucible is made of: | Porcelain |
| Sintered glass is a porous material used for: | Filtration |
| A suitable solvent should dissolve the maximum amount of solute at its boiling point and a minimum amount at: | Room temperature |
| 95% ethanol is called: | Rectified spirit |
| The solution left after the formation of crystals is called: | Mother liquor |
| Which one of the following substances is not used as a drying agent in desiccators? | NaCl (50%) |
| Which one of the following substances is used as a decolorizing agent? | Animal charcoal |
| Question | Answer |
| In primary alkyl halides, the halogen atom is attached to a carbon which is attached to how many carbon atoms? | One |
| The reactivity order of alkyl halides for a particular alkyl group is: | I > Br > Cl > F |
| When CO2 is made to react with ethyl magnesium iodide, followed by hydrolysis, the product formed is: | Propanoic acid |
| Grignard reagent is reactive due to: | The polarity of C-Mg bond |
| SN2 reactions can be best carried out with: | Primary alkyl halide |
| Elimination bimolecular reactions involve: | Second order kinetics |
| For which mechanisms, the first step involved is the same: | E1 and SN1 |
| Alkyl halides are considered to be very reactive compounds towards nucleophiles, because: | They have an electrophilic carbon and good leaving group |
| The rate of E1 reaction depends upon: | The concentration of substrate |
| Which one of the following is not a nucleophile? | BF3 |
| General formula of alkyl halide is: | R-X |
| General formula of alkyl halide is: | CnH2n+1X |
| Best method of preparation of alkyl halide from alcohols is by its reaction with: | All |
| Alkyl halides are reactive: | High |
| SN2 reaction has order of reaction: | Second |
| E2 has molecularity: | 2 |
| The conversion of n-hexane into benzene by heating in the presence of Cr2O3 is called: | Aromatization |
| Simplest aromatic compound is: | Benzene |
| Ratio of carbon to hydrogen in aromatic compounds is: | High than alkanes |
| Kekule structures contributed towards actual structure of benzene: | 60% |
| Resonance energy of benzene is (in KJ mol-1): | 150 |
| Benzene gives reactions generally: | Electrophilic substitution |
| Which decolourises the colour of Br2? | (b) and (c) |
| Which is symmetrical alkene? | (b) and (c) |
| Free radical mechanism of halogenation of alkanes follow step: | All of these |
| Alkanes have functional group: | No functional group |
| Which is the more reactive? | Alkynes |
| Acetylene can be converted into while passing through a Cu-tube at 300°C. | Benzene |
| Odour of alkyne is: | Garlic like |
| Alkene general formula: | CnH2n |
| Alkyne is: | CH≡CH |
| Alkanes are gases: | C1-C4 |
| The benzene molecule contains: | Delocalized π electron charge |
| Aromatic hydrocarbons are the derivatives of: | Benzene |
| Which of the following acid can be used as a catalyst in Friedel Craft’s reactions? | HCl |
| Benzene cannot undergo: | Addition reactions |
| Amongst the following, the compound that can be most readily sulphonated is: | Toluene |
| During nitration of benzene, the active nitrating agent is: | NO2+ |
| Acylation of benzene to produce aliphatic aromatic ketones is known as: | Friedel Craft’s reaction |
| Benzene reacts with Cl2 in sunlight to give the end product: | C6H6Cl6 |
| Which of following is explosive? | Nitrobenzene |
| Which compound is the most reactive one? | Ethyne |
| Among the following, polycyclic compound is: | Naphthalene |
| Benzene can be obtained from: | All |
| The electrophile in aromatic sulphonation is: | SO3 |
| Aromatic compounds burn with sooty flame cause: | They have high percentage of carbon |
| Question | Answer |
| The carbon of a carbonyl group is: | sp² hybridized |
| Formalin is: | 40% solution of formaldehyde in water |
| Which of the following will have the highest boiling point? | 2-Hexanone |
| Ketones are prepared by the oxidation of: | Secondary alcohol |
| Acetone reacts with HCN to form a cyanohydrin. It is an example of: | Nucleophilic addition |
| Which of the following compounds will not give Iodoform test on treatment with I2/NaOH? | 3-Pentanone |
| Which of the following compounds will react with Tollen’s reagent? | CH3COCH |
| Cannizzaro’s reaction is not given by: | Acetaldehyde |
| Which of the following reagent will react with both aldehyde and ketone? | Grignard’s reagent |
| Aldehydes are oxidized to give: | Carboxylic acid |
| Carboxyl compounds have functional group: | R-CH=O |
| The homologous series of aldehydes and ketones have general formula: | CnH2O |
| Formula of acetone is: | CH3COCH3 |
| Reaction of Grignard’s reagent with formaldehyde gives: | Primary alcohol |
| Reaction of Grignard’s reagent with aldehydes other than formaldehyde gives: | Secondary alcohol |
| Reaction of Grignard’s reagent with ketones gives: | Tertiary alcohol |
| Iodoform test is given by: | Acetaldehyde and methyl ketones |
| Aldehydes and ketones can be prepared from alcohols by their: | Oxidation |
| Common names of aldehydes are given by corresponding: | Carboxylic acid |
| Cannizzaro’s reaction is type of reaction: | Self oxidation-Reduction reaction |
| Acetic acid is manufactured by: | Fermentation |
| Metal used in the preparation of Grignard’s reagent is: | Mg |
| Reaction of Grignard’s reagent with CO2 gives: | Carboxylic acid |
| Reaction of which with Grignard’s reagent gives primary alcohol: | Formaldehyde |
| Primary carbon attaches with other hydrogen atoms directly: | At least one or more than it |
| Which compound shows more hydrogen bonding? | C2H5OH |
| Which compound shows maximum hydrogen bonding with water? | CH3OH |
| Which compound is more soluble in water? | CH3OH |
| Which compound will have the maximum repulsion with water? | CH4 |
| Ethanol can be converted into ethanoic acid by: | Oxidation |
| Which enzyme is not involved in the fermentation of starch? | Urease |
| Which compound is called a universal solvent? | H2O |
| Methyl alcohol is not used: | As a substitute for petrol |
| Rectified spirit contains alcohol about: | 95% |
| According to Lewis concept ethers behave as: | Base |
| Phenols are derivatives of: | Benzene |
| Alcohols are derivatives of: | Alkanes |
| Derivative of water is: | All of these |
| Dow’s method is used to prepare: | Phenol |
| Which is not a property in ether: | High boiling point |
| Methanol is prepared from CO and H2 using catalyst: | ZnO |
| Taste of lower alcohols is: | Sweet |
| Oxidation of tertiary alcohol gives: | Alkenes |
| Alcohols can be distinguished using test: | Lucas |
| Ethyl alcohol prepared during fermentation is pure: | 12% |
| Question | Answer |
| In which of these processes are small organic molecules made into macromolecules? | The polymerization of ethane |
| Which of these polymers is an addition polymer? | Polystyrene |
| Which of these polymers is a synthetic polymer? | Polyester |
| Plastics are a pollution problem because many plastics: | Burn to produce toxic fumes |
| The fiber which is made from acrylonitrile as monomer: | Acrylic fibre |
| A polymeric substance that is formed in the liquid state and then hardened to a rigid solid is called a: | Plastic |
| Vegetable oils are: | Glycerides of unsaturated fatty acids |
| Which one of the following elements is not present in all proteins? | Sulphur |
| Which one of the following is a water-soluble vitamin? | Ascorbic acid |
| Which one of the following enzymes brings about the hydrolysis of fats? | Lypase |
| The reaction between fat and NaOH is called: | Saponification |
| Which one of the following statements about glucose and sucrose is incorrect? | Both are disaccharides |
| Which behaves as an insulator for the animal’s body? | Fats |
| The steroids of fungi and yeast are called: | Ergosterol |
| An oil or fat with no double bond has an iodine number: | Zero |
| Which property is not present in lipids? | Soluble in water |
| Which is the derived lipid? | Vitamin-D |
| Major food factors are: | All of these |
| Factors affecting denaturation of proteins: | All of these |
| The high molecular weight materials which yield on hydrolysis the amino acids is called: | Proteins |
| Cement is a combination of mainly: | Calcareous and argillaceous |
| Major component in cement is: | Lime |
| Composition of clay in cement is: | 25% |
| Pakistan in the beginning was a country: | Agrarian |
| Which is not a nitrogenous fertilizer? | Calcium phosphate |
| A carboxylic acid contains: | A hydroxyl and carbonyl group |
| Which acid is used in the manufacture of synthetic fibre? | Acetic acid |
| Which following derivative cannot be prepared directly from acetic acid? | Acetamide |
| Which reagent is used to reduce a carboxylic group to an alcohol? | LiAlH4 |
| The solution of which acid is used for seasoning of food? | Acetic acid |
| Organic compounds X and Y react together to form organic compound Z. What types of compounds can X, Y, and Z be? | X: Alcohol, Y: Acid, Z: Ester |
| An aqueous solution of an organic compound reacts with sodium carbonate to produce carbon dioxide gas. Which one of the following could be the organic compound? | CH3CH2COOH |
| Which of the following is not a fatty acid? | Phthalic acid |
| Acetamide is prepared by: | Heating ammonium acetate |
| A carboxylic acid with one carboxyl group: | Monocarboxylic acid |
| A compound containing a carboxyl group in them is called: | Carboxylic acids |
| A carboxylic acid containing Ar group in it is called: | Aromatic carboxylic acid |
| O-COOH is an example of carboxylic acid: | Aromatic carboxylic |
| In preparation method of carboxylic acids from alkyl halide always carboxylic acid formed which have carbon atoms: | One more than in R-X |
| Which is not a carboxylic acid with a pungent smell? | Ethanoic acid |
| Carboxyl group has functional groups in it: | One |
| Carboxylic acids react with acids releasing gas from it: | CO2 |
| Active metals react with carboxylic acids releasing gas: | H2 |
| Acetic acid reacts with PCl5 giving: | Acetyl chloride |
| Question | Answer |
| The branch of science dealing with structure, composition, and changes in matter and the laws and principles governing these changes is called? | Chemistry |
| Smallest particle of an element which may or may not have independent existence is known as? | An atom |
| Matter is defined as anything which occupies space and? | Mass |
| The number of atoms present in a molecule determines its? | Atomicity |
| When an electron is added to a unipositive ion we get? | Neutral atom |
| CO is an example of? | Stable molecule |
| The diameter of atoms is of the order? | 2 x 10⁻¹⁰ m |
| Swedish chemist J. Berzelius determined? | Atomic mass |
| Covalent compounds mostly exist in the form of? | Molecules |
| Atoms and molecules can either gain or lose electrons, forming charged particles called? | Ions |
| Metals tend to lose electrons, becoming? | Positively charged ions |
| Non-metals tend to gain electrons, becoming? | Negatively charged ions |
| First atomic theory was put forward by an English school teacher? | John Dalton |
| Determination of atomic masses and invention of the system of writing symbols was made by? | Berzelius |
| Atoms can be evident by the use of electron microscope, field ionization microscope, and? | X-rays |
| The number of subatomic particles in atoms so far discovered is more than? | 100 |
| C₂H₂O₄ and C₄H₄O₄ are? | Poly-atomic molecules |
| Cl₂, N₂, and O₂ are? | Diatomic molecules |
| He, Ar, and Ne are? | Mono-atomic molecules |
| NH₃, HCl, H₂O, HI are? | Poly-atomic molecules |
| The pH range of acid rain is? | Less than 5 |
| Peroxyacetyl nitrate (PAN) is an irritant to human beings and it affects? | Eyes |
| The range of UV-B is? | 280 to 320 nm |
| A single chloride free radical can destroy how many ozone molecules? | 100000 |
| Fungicides are the pesticides which? | Control the growth of fungus |
| DDT is a? | Insecticide |
| The main pollutant of leather tanneries in the wastewater is due to the salt of? | Chromium (VI) |
| In purification of potable water, the coagulant used is? | Aluminium sulphate |
| The temperature in the incineration process has a range? | 950 to 1300°C |
| Newspaper can be recycled again and again by how many times? | 5 |
| Chloroform is carcinogenic to? | Liver |
| Which is used as a coagulant? | Ferric salts and Potash alum |
| Water is purified by the process? | All of these |
| BOD is the oxygen demand within how many days? | Five |
| Factors affecting the quality of water? | DO, BOD, COD |
| Contamination of water of tanning industries is due to? | Cr(VI) |
| Forms of waste products? | All of these |
| How many pesticides have been synthesized at present? | Ten thousand |
| A single free chlorine radical can destroy ozone molecules up to? | 100000 |
| Depletion of ozone is more during the month? | Sept-Nov |
| Unit of ozone is? | Dobson |
| Main cause of reducing smog is? | All of these |
| Coal contains sulfur in it? | 1-6% |
| Volcanoes produce SO₂? | 67% |
| Reasons for pollution are? | All of these |
| Question | Answer |
| Which statement is true about order of reaction? | Order of reaction can only be determined by an experiment |
| The unit of rate constant K is mole⁻¹ dm³ s⁻¹ for a chemical reaction, the order of reaction is? | 2 |
| Hydrolysis of ethyl-acetate (ester) has order of reaction? | 2 |
| If rate law of an equation is written as -dx/dt = k[A][B]²? | Reactant is decreasing with passage of time |
| The example of a photochemical reaction is photosynthesis has order of reaction? | 0 |
| Rate law of an equation is obtained? | Experimentally |
| A pseudo uni-molecular reaction has order of reaction? | 1 |
| A zero order reaction is one in which? | Rate is not affected by changing concentration of reactants |
| The rate equation for a reaction is Rate = K[A]. What are units of K? | mol dm⁻³ s⁻¹ |
| The unit of the rate constant is the same as that of rate of reaction in? | Zero order reaction |
| Half life period of a first order reaction is independent of? | All of above |
| If the rate of decay of radioactive isotope decreases from 200 cpm to 25 cpm after 24 hours, what is its half-life? | 8 hours |
| The rate of reaction between two specific time intervals is called? | Average rate of reaction |
| Dilatometer method is useful for the reaction that involve? | Small volume changes in solutions |
| The rate of reaction? | Decreases as the reaction proceeds |
| Keeping in view the size of atoms, which order is the correct one? | Cl < I |
| Mark the correct statement. | Na⁺ is smaller than Na atom |
| Mark the correct statement. | All the alkali metals are present in the same group |
| Which statement is incorrect? | All the metals form acidic oxides |
| Which statement is correct? | Hydrogen resembles in properties with I-A, VII-A and IV-A elements |
| Mark the correct statement. | The ionization energy of calcium is higher than that of beryllium |
| Mark the correct statement. | Electron affinity is a measure of energy released by removing an electron |
| Mark the incorrect statement. | Metallic character remains the same down the group |
| Mark the correct statement. | Melting points of halogens first increase and then decrease down the group |
| Mark the correct statement. | Covalent character of metal halides increases from left to right in a period |
| Modern Periodic Table is based upon periods function? | Atomic number |
| Newland’s gave law? | Octaves law |
| The element not known till Mendeleev tabulated his periodic table? | Germanium |
| Which one was the problem associated with Mendeleev periodic table? | Grouping of alkali metals with coinage metals |
| BOD is the oxygen demand within day(s)? | Five |
| Question | Answer |
| (A) is one molar NaCl solution and (B) is molal NaCl solution: | B is more concentrated than A |
| A solution of sucrose is 34.2%. The volume of solution containing one mole of solute: | 1000 cm³ |
| 10g of NaOH has been dissolved per dm³ of solution. The molarity of solution is: | 0.25 M |
| 10g of NaOH has been dissolved per kg of solvent. The molality of solution is: | 0.25 m |
| The sum of mole per cent of all the components of solution is always equal to: | 100 |
| The ratio of moles of a particular component of solution to total moles of all components of solution is: | Mole fraction |
| 5g of glucose is dissolved for 100 cm³ of solution. The percentage of solution is: | 5% w/v |
| Electrochemistry is concerned with the conversion of electrical energy into chemical energy in: | Electrolytic cell |
| The conversion of chemical energy into electrical energy requires: | Both Galvanic cell and Voltaic cell |
| Most metals are conductors of electricity because of the: | Relatively free movement of their electrons |
| Metallic conduction is also called as: | Electronic conduction |
| Electrolytes in the form of solution or in the fused state have the ability to conduct: | Ions |
| Ionization is the process in which ionic compounds when fused or dissolved in water split up into charged particles called: | Ions |
| Electrolysis is used for: | All of above |
| In an electrolytic cell, the electrons flow from: | Anode to cathode |
| When aqueous NaCl is electrolyzed, which of the following ions get discharged at anode: | Cl⁻ |
| In electrolytic cells, the chemical changes may be: | Either spontaneous or non- spontaneous |
| Which of the following cannot conduct electricity: | NaCl (fused) |
| During electrolysis, the reaction that takes place at cathode is: | Reduction |
| During electrolysis, electrons are: | Gained by cathode |
| The function of salt bridge is: | To maintain electrical neutrality |
| Which of the following yield both hydrogen and chlorine on electrolysis: | Electrolysis of aqueous NaCl |
| Which of the following correctly describes the process occurring at the electrodes when molten NaCl is electrolyzed: | Oxidation at anode, reduction at cathode |
| What are the products of electrolysis of aqueous sodium chloride at two electrodes: | Chlorine at anode and hydrogen at cathode |
| Sodium can be obtained by: | Electrolysis of molten sodium chloride |
| A cell in which electric current is produced as a result of spontaneous redox reaction is called: | Galvanic cell |
| A cell which produces electrical current by an oxidation-reduction reaction is known as: | Voltaic cell |
| Which of the following reactions occur at moderate rate: | Rusting of iron |
| All reactions occur in: | Both a single step and a series of steps |
| The rate determining step is the: | Slowest step |
| Which of the following will affect the rate: | Rate determining step |
| It is common observation that rates of chemical reactions differ: | Greatly |
| Which of the following may affect the rate constant (K) for a reaction: | Change in temperature |
| The change in concentration of reactant or product per unit time is called: | Rate of reaction |
| Rate of a chemical reaction depends upon: | Number of fruitful collisions per second |
| Question | Answer |
| A reaction is reversible because: | Products are reactive |
| What happens when a reaction is at equilibrium and more reactant is added: | Forward reaction rate is increased |
| The rate of a chemical reaction is directly proportional to product of molar concentration of reacting substance. It is called: | Law of mass action |
| A chemical reaction A ⇌ B is said to be in equilibrium when: | Rate of transformation of A to B is equal to B to A |
| The rate of reaction: | Remains same as reaction proceeds |
| Law of mass action was given by: | Guldberg and Waage |
| In a chemical reaction equilibrium is said to have been established when: | Rate of opposing reactions are equal |
| In the above equilibrium system, if the concentration of reactants at 25°C is increased, the value of Kc will: | Remains constant |
| For the above reaction the relationship between Kc and Kp will be: | Kp = Kc(RT)^-1 |
| The correct relation between Kc and Kp is: | Kp = Kc(RT)^Δn |
| N₂O₄ ⇌ 2NO₂ 1 mol of N₂O₄ was decomposed according to given equation in 1dm³ container. At equilibrium x mole of N₂O₄ have dissociated. What is the value of Kc: | 4x² / (1-x) |
| 2NO ⇌ N₂ + O₂ The unit of Kc for this reaction will be: | No unit |
| N₂ + 3H₂ ⇌ 2NH₃ The unit of Kc for this reaction will be: | mol⁻² dm⁶ |
| For what value of Kc almost forward reaction is complete: | Kc = 10³ |
| In a particular reaction for the value Kc = 1 x 10³⁰ which statement is correct: | Almost forward reaction is complete |
| Almost forward reaction is complete when value of Kc is: | Very large |
| If Kc of a reaction is very large, it indicates that equilibrium occurs: | At a high product concentration |
| N₂O₄ ⇌ 2NO₂ For the above reaction, which of the following expression of Kc is correct: | Kc = [NO₂]² / [N₂O₄] |
| In an exothermic reversible reaction increase in temperature shift the equilibrium to: | Reactant side |
| A large value of K means that at equilibrium: | Less reactants and more products |
| Every sample of matter with uniform properties and a fixed composition is called a: | Phase |
| A solution is a homogeneous mixture of two or more kinds of different: | Ionic substances |
| The substance which is present in large quantity is called a: | Solvent |
| The substance which is present in small quantity is called as: | Solute |
| Solutions containing relatively lower concentrations of solute are called: | Dilute solutions |
| In which type of following solutions we don’t know the total volume of the solution: | Percentage weight/weight |
| In which of the following solutions the total volume of solution may not be necessarily equal to sum of volumes of solute and solvent? | Percentage volume/volume |
| The number of moles of solute dissolved per dm³ of the solution is called: | Molarity |
| The number of moles of solute in 1000g (1 kg) of the solvent is called: | Molality |
| As compared to molar solution, in the molal solution the quantity of solvent is: | Comparatively greater |
| To calculate volume of the solvent, we need to know, the: | Mass of solute |
| Molarity of pure water is: | 55.5 |
| A solution of glucose is 10%. The volume to which 1g mole of it dissolved will be: | 1.8 dm³ |
| Question | Answer |
| The study of heat changes accompanying a chemical reaction is known as: | Thermochemistry |
| If an endothermic reaction is allowed to take place very rapidly in air, the temperature of the surrounding air: | Decreases |
| In endothermic reactions, the heat contents of the: | Products more than that of reactants |
| The majority of reactions which give stable products are: | Exothermic |
| It is noticed that energy in the form of heat is either evolved or absorbed as a result of a: | Chemical change |
| In a chemical change, the energy in the form of heat will either be evolved or absorbed and this is called: | Heat of reaction |
| The energy units in which heat changes usually expressed in SI-system are: | Joule |
| The subject matter of first law of thermochemistry is based on: | First law of Thermodynamics |
| A process which takes place on its own from a non-equilibrium state towards an equilibrium state is termed as: | Both Spontaneous and Natural process |
| Which one of the following is not related to spontaneous process: | Artificial |
| Neutralization of a strong acid with a strong base is: | Both Natural acid base reaction and Spontaneous acid base reaction |
| When a piece of zinc is added to the copper sulphate solution, colour of solution disappear: | Blue |
| The reaction of Zinc with copper sulphate solution is an example of: | Spontaneous redox reaction |
| A reaction will also be called a spontaneous if: | It does not need energy to start with |
| Burning of coal and hydrocarbon in air are examples of: | Both Spontaneous reaction and Natural reaction |
| Some non-spontaneous processes can be made to take place by supplying energy to the system from: | All of above |
| By state, we mean the: | Condition of a system |
| When no work is done by the system: | The volume of system decreases |
| When a system absorbs energy, the sign of ΔE is: | Positive |
| Work is a: | Only function |
| The real or imaginary surface separating the system from the surroundings is called: | Boundary |
| One mole of oxygen confined in a cylinder fitted with a piston is an example of: | System |
| Reaction between Zn and CuSO4 can be called a system under: | Observation |
| By comparing both initial and final states of the system, we can describe the change taking place in the: | System |
| A state function is a: | Macroscopic property |
| Which one of the following is not a state function? | Heat |
| The kinetic energy is due to: | All of above (Translational, Rotational, Vibrational movements) |
| Potential energy accounts for: | All types of attractive forces present in system |
| The total of all the possible kinds of energies of the system is called its: | Internal energy |
| ΔE is a: | State function |
| Heat is: | Not a property of the system |
| Heat evolved or absorbed by the system is represented by a symbol: | q |
| The SI unit of work is: | Joules |
| The kind of work most commonly encountered in chemistry is: | Pressure volume work |
| Internal energy of the system is an: | Extensive property |
| The increase in internal energy of a system can result in: | Both Physical change and Chemical change |
| Heat evolved by a system is given: | Negative sign |
| Energy of universe remains constant. It is called: | First law of Thermodynamics |
| First law of thermodynamics is represented as: | ΔE = q + w |
| Which of the following statements is contrary to the first law of thermodynamics: | Continuous production of mechanical work without supplying equivalent amount of heat is possible |
