1. Which of the following is not a state function?

(a) \(q_p\)

(b) \(q\)

(c) enthalpy

(d) entropy.

2. Which of the following is not an extensive property?

(a) molarity

(b) heat capacity

(c) mass

(d) volume.

3. In a chemical reaction work is done by the system when

(a) number of moles of gaseous reactants is equal to the number of moles of gaseous products

(b) total number of moles increases

(c) number of moles of gaseous substances decreases

(d) number of moles of gaseous products is greater than the number of moles of gaseous reactants.

4. The heat evolved in the following reaction \(2 \mathrm{H}_2(\mathrm{~g})+\mathrm{O}_2(\mathrm{~g}) \longrightarrow 2 \mathrm{H}_2 \mathrm{O}(\mathrm{1}), \Delta \mathrm{H}=-484 \mathrm{~kJ}\) to produce \(9 \mathrm{~g}\) of water is

(a) \(484 \mathrm{~kJ}\)

(b) \(121 \times 10^3 \mathrm{~J}\)

(c) \(242 \mathrm{~kJ}\)

(d) \(968 \mathrm{~kJ}\)

5. When a sample of an ideal gas is allowed to expand at constant temperature against an atmospheric pressure,

(a) surroundings does work on the system

(b) \(\Delta \mathrm{U}=0\)

(c) no heat exchange takes place between the system and surroundings

(d) internal energy of the system increases.

6. In what reaction of the following, work is done by the system on the surroundings?

(a) \(\mathrm{Hg}(\mathrm{l}) \longrightarrow \mathrm{Hg}(\mathrm{g})\)

(b) \(3 \mathrm{O}_2\) (g) \(\longrightarrow 2 \mathrm{O}_3\) (g)

(c) \(\mathrm{H}_2(\mathrm{~g})+\mathrm{Cl}_2(\mathrm{~g}) \longrightarrow 2 \mathrm{HCl}(\mathrm{g})\)

(d) \(\mathrm{N}_2(\mathrm{~g})+3 \mathrm{H}_2(\mathrm{~g}) \longrightarrow 2 \mathrm{NH}_3(\mathrm{~g})\)

7. A gas does \(0.320 \mathrm{~kJ}\) of work on its surroundings and absorbs \(120 \mathrm{~J}\) of heat from the surroundings. Hence, \(\Delta U\) is

(a) \(440 \mathrm{~kJ}\)

(b) \(200 \mathrm{~J}\)

(c) \(120.32 \mathrm{~J}\)

(d) \(-200 \mathrm{~J}\)

8. In the reaction, \(\mathrm{H}_2(\mathrm{~g})+\mathrm{Cl}_2(\mathrm{~g}) \longrightarrow 2 \mathrm{HCl}(\mathrm{g}) \Delta \mathrm{H}\) \(=-184 \mathrm{~kJ}\), if 2 moles of \(\mathrm{H}_2\) react with 2 moles of \(\mathrm{CI}_2\), then \(\Delta \mathrm{U}\) is equal to

(a) \(-184 \mathrm{~kJ}\)

(b) \(-368 \mathrm{~kJ}\)

(c) Zero

(d) \(+368 \mathrm{~kJ}\)

9. For which of the following substances \(\Delta_l H^{\circ}\) is not zero

(a) \(\mathrm{Ca}\) (s)

(b) \(\mathrm{He}(\mathrm{g})\)

(c) \(\mathrm{P}\) (red)

(d) \(\mathrm{CH}_3 \mathrm{OH}(1)\)

10. If for a reaction \(\Delta H\) is negative and \(\Delta S\) is positive then the reaction is

(a) spontaneous at all temperatures

(b) nonspontaneous at all temperatures

(c) spontaneous only at high temperatures

(d) spontaneous only at low temperatures

11. The relationship between \(\Delta G^6\) of a reaction and its equilibrium constant is

(a) \(-\Delta G^0=\frac{R T}{\ln K}\)

(b) \(\Delta \mathrm{G}^0=\frac{R T}{\ln \mathrm{K}}\)

(c) \(\frac{\mathrm{RT} \ln \mathrm{K}}{\Delta \mathrm{G}^0}=-1\)

(d) \(\Delta G^{\circ}=\) RT \(\ln \mathrm{K}\)

12. Which of the following has highest entropy?

(a) \(\mathrm{Al}(\mathrm{s})\)

(b) \(\mathrm{CaCO}_3\) (s)

(c) \(\mathrm{H}_2 \mathrm{O}\) (1)

(d) \(\mathrm{CO}_2(\mathrm{~g})\)

13. For the process, \(\mathrm{H}_2 \mathrm{O}(1) \longrightarrow \mathrm{H}_2 \mathrm{O}(\mathrm{g})\) at \(100^0 \mathrm{C}\), \(\Delta S\) is

(a) positive

(b) negative

(c) zero

(d) unpredictable

14. For the conversion of liquid to solid below the melting point of solid

(a) \(\Delta S_{\mathrm{ms}}\) is negative and the process is spontaneous

(b) \(\Delta \mathrm{S}_{\mathrm{m}}\) is positive and the process is spontaneous

(c) \(\Delta \mathrm{S}_{\mathrm{var}}\) is positive and the process is nonspontaneous

(d) \(\Delta S_{m s}\) is zero and the process is at equilibrium.

15. Which of the following conditions guarantee that a reaction is spontaneous at constant \(T\) and \(P\) ?

(a) entropy of system increases

(b) enthalpy of system decreases

(c) entropy of system decreases and that of surroundings increases

(d) Gibbs energy of the system decreases.

16. Which of the following processes is nonspontaneous?

(a) dissolving \(\mathrm{KCl}\) in water

(b) mixing of iodine vapour and nitrogen gas

(c) decomposition of \(\mathrm{NaCl}\) to \(\mathrm{Na}\) (s) and \(\mathrm{Cl}_2(\mathrm{~g})\)

(d) freezing of water at \(270 \mathrm{~K}\).

17. For which of the following' reactions \(\Delta S\) is negative?

(a) \(\mathrm{Mg}(\mathrm{s})+\mathrm{Cl}_2\) (g) \(\longrightarrow \mathrm{MgCl}_2\) (s)

(b) \(\mathrm{H}_2 \mathrm{O}(\mathrm{l}) \longrightarrow \mathrm{H}_2 \mathrm{O}(\mathrm{g})\)

(c) \(\mathrm{CaCO}_3\) (s) \(\longrightarrow \mathrm{CaO}\) (s) \(+\mathrm{CO}_2\) (g)

(d) \(\mathrm{I}_2(\mathrm{~g}) \longrightarrow 2 \mathrm{I}(\mathrm{g})\)

18. A gas expands in volume from \(2 \mathrm{~L}\) to \(5 \mathrm{~L}\) against a pressure of 1 atm at constant temperature. The work done by the gas will be

(a) \(3 \mathrm{~J}\)

(b) \(-303.9 \mathrm{~J}\)

(c) \(-303.9 \mathrm{~L}\).atm

(d) \(303.9 \mathrm{~L}\) atm

19. Given the reaction,

The enthalpy of formation of \(\mathrm{NH}_3\) is

(a) \(-92.6 \mathrm{~kJ}\)

(b) \(92.6 \mathrm{~kJ} \mathrm{~mol}^{-1}\)

(c) \(-46.3 \mathrm{~kJ} \mathrm{~mol}^{-1}\)

(d) \(-185.2 \mathrm{~kJ} \mathrm{~mol}^{-1}\)

20. Which of the following compounds will absorb maximum quantity of heat when dissolved in the same amount of water. The enthalpies of solution of these compounds at \(25^{\circ} \mathrm{C}\) in k.J \(/\) mole are given in brackets ?

(a) \(\mathrm{P}\left(\Delta \mathrm{H}=-32.6 \mathrm{~kJ} \mathrm{~mol}^{-1}\right)\)

(b) \(\mathrm{Q}\left(\Delta \mathrm{H}=-17.3 \mathrm{~kJ} \mathrm{~mol}^{-1}\right)\)

(c) \(\mathrm{R}\left(\Delta \mathrm{H}=+2.56 \mathrm{~kJ} \mathrm{~mol}^{-1}\right)\)

(d) \(\mathrm{S}\left(\Delta \mathrm{H}=+25.6 \mathrm{~kJ} \mathrm{~mol}^{-1}\right)\)

21. For a reversible process at equilibrium, the change in entropy may be expressed as

(a) \(\Delta \mathrm{S}=\mathrm{Tq}_{\mathrm{rev}}\)

(b) \(\Delta \mathrm{S}=\frac{\mathrm{q}_{\mathrm{rev}}}{\mathrm{T}}\)

(c) \(\Delta S=\frac{\Delta H}{T}\)

(d) \(\triangle \mathrm{S}=\Delta \mathrm{G}\).

22. Free energy, may be defined as :

(a) \(\mathrm{G}=\mathrm{U}-\mathrm{TS}\)

(b) \(\mathrm{G}=\mathrm{U}+\mathrm{TS}\)

(c) \(\mathrm{G}=\mathrm{H}-\mathrm{TS}\)

(d) \(\mathrm{G}=\mathrm{U}+\mathrm{H}-\mathrm{TS}\).

23. When a solid changes into liquid, the entropy

(a) increases

(b) remains the same

(c) decreases

(d) becomes zero.

24. If \(q\) is the heat added to the system, \(W\) is the work done by the system and \(\triangle E\) is the change in internal energy, then according to first law of thermodynamics

(a) \(\Delta \mathrm{U}=\mathrm{q}+\mathrm{w}\)

(b) \(\Delta \mathrm{U}=\mathrm{q}-\mathrm{w}\)

(c) \(\Delta \mathrm{U}=\mathrm{q}+\mathrm{p} \Delta \mathrm{V}\)

(d) \(\Delta \mathrm{U}=\mathrm{q}+\Delta \mathrm{H}\)

25. Which of the following pairs has heat of neutralisation equal to \(-57.1 \mathrm{k} \mathbf{J}\) ?

(a) \(\mathrm{HNO}_3, \mathrm{KOH}\)

(b) \(\mathrm{HCl}, \mathrm{NH}_4 \mathrm{OH}\)

(c) \(\mathrm{H}_2 \mathrm{SO}_4, \mathrm{NH}_4 \mathrm{OH}\)

(d) \(\mathrm{CH}_3 \mathrm{COOH}, \mathrm{NaOH}\).

26. Free energy is related to enthalpy and entropy changes as

(a) \(\Delta \mathrm{G}=\Delta \mathrm{H}-\mathrm{T} \Delta \mathrm{S}\)

(b) \(\Delta \mathrm{G}=\mathrm{T} \Delta \mathrm{S}-\Delta \mathrm{H}\)

(c) \(\Delta \mathrm{G}=\frac{\Delta \mathrm{H}-\Delta \mathrm{S}}{\mathrm{T}}\)

(d) \(\Delta \mathrm{G}=\Delta \mathrm{H}+\mathrm{T} \Delta \mathrm{S}\)

27. A spontaneous change is one in which the system suffers

(a) Increase in internal energy

(b) Lowering of entropy

(c) Lowering of free energy

(d) No energy change

28. For which of the following reactions, \(\Delta S\) is not positive?

(a) \(\mathrm{I}_2(\mathrm{~s}) \rightarrow \mathrm{I}_2\) (g)

(b) \(\mathrm{CuO}(\mathrm{s})+\mathrm{H}_2\) (g) \(\rightarrow \mathrm{Cu}(\mathrm{s})+\mathrm{H}_2 \mathrm{O}(\ell)\)

(c) \(2 \mathrm{O}_3\) (g) \(\rightarrow 3 \mathrm{O}_2(\mathrm{~g})\)

(d) \(\mathrm{CH}_4\) (g) \(+2 \mathrm{O}_2\) (g) \(\rightarrow \mathrm{CO}_2\) (g) \(+\mathrm{H}_2 \mathrm{O}\) (g).

29. For an equilibrium state,

(a) \(\Delta \mathrm{H}>0\)

(b) \(\Delta \mathrm{G}>0\)

(c) \(\Delta \mathrm{H}=\mathrm{T} \Delta \mathrm{S}\)

(d) \(\Delta \mathrm{H}>\mathrm{T} \Delta \mathrm{S}\).

30. If there is no exchange of heat between the system and the surrounding during the process, it is called

(a) Isobaric process

(b) adiabatic process

(c) isothermal process

(d) irreversible process.

31. For the reaction, \(\mathrm{PCl}_5(\mathrm{~g}) \rightarrow \mathrm{PCl}_3(\mathrm{~g})+\mathrm{Cl}_2(\mathrm{~g})\)

(a) \(\Delta \mathrm{H}=\Delta \mathrm{U}\)

(b) \(\Delta \mathrm{H}>\Delta \mathrm{U}\)

(c) \(\Delta \mathrm{H}<\Delta \mathrm{U}\)

(d) None of the above.

32. An endothermic reaction is allowed to occur veryrapidly in the air. The temperature of the surrounding air

(a) remains constant

(b) decreases

(c) increases

(d) may increase or decrease.

33. Which of the following is not an intensive property ?

(a) Entropy

(b) Pressure

(c) Temperature

(d) Molar volume.

34. Which of the following is not a state function ?

(a) Heat

(b) Internal energy

(c) Enthalpy

(d) Entropy

35. For a chemical reaction at constant \(\mathbf{P}, \mathbf{\Delta H}\) is equal to

(a) zero

(b) \(\omega\)

(c) \(q / T\)

(d) \(\mathrm{zu}+\mathrm{p} \Delta \mathrm{V}\)

36. The enthalpy change for the process: \(\mathrm{C}(\mathrm{s}) \rightarrow \mathbf{C}(\mathrm{g})\) corresponds to enthalpy of

(a) fusion

(b) sublimation

(c) combustion

(d) vaporisation.

37. In an electrochemical cell, if \(\mathbf{E}\) is the e.m.f. of the cell involving \(\mathrm{n}\) mole of electrons, then \(\Delta G^0\) is

(a) \(\Delta \mathrm{G}^0=n \mathrm{nFE}^\theta\)

(b) \(\Delta \mathrm{G}^0=-\mathrm{nFE}\)

(c) \(\mathrm{E}^0=\mathrm{nF} \Delta \mathrm{G}^0\)

(d) \(\Delta \mathrm{G}^0=\frac{n F}{E^0}\)

38. For a spontaneous endothermic reaction:

(a) \(\Delta \mathrm{G}>0\)

(b) \(\Delta \mathrm{G}=0\)

(c) \(\Delta \mathrm{H}<0\)

(d) \(\Delta \mathrm{S}>\frac{\Delta \mathrm{H}}{\mathrm{T}}\)

39. For the reversible vaporisation of water at 373 \(\mathrm{K}\) and 1 atmospheric pressure, \(\Delta \mathrm{G}\) is equal to

(a) \(\Delta \mathrm{H}\)

(b) \(\triangle \mathrm{S}\)

(c) zero

(d) \(\Delta \mathrm{H} / \mathrm{T}\)

40. For a chemical reaction at constant \(P\) and \(V\), \(\Delta \mathrm{H}\) is equal to

(a) \(\Delta \mathrm{U}\)

(b) zero

(c) \(\Delta \mathrm{U}+\mathrm{P} \Delta \mathrm{V}\)

(d) \(\mathrm{p} / \mathrm{T}\)

41. \((\Delta \mathrm{U}-\Delta \mathrm{H})\) for the formation of \(\mathrm{NH}_3\) from \(\mathrm{N}_2\) and \(\mathrm{H}_2\) is

(a) \(-2^2 \mathrm{RT}\)

(b) \(2 \mathrm{RT}\)

(c) RT

(d) \(\frac{1}{2} \mathrm{RT}\)

42. The sign of \(\Delta \mathrm{G}\) for the process of melting of ice at \(260 \mathrm{~K}\) is

(a) \(\Delta \mathrm{G}=0\)

(b) \(\Delta \mathrm{G}<0\)

(c) \(\Delta \mathrm{G}>0\)

(d) None of these

43. A system absorbs \(\mathbf{1 0} \mathrm{k} . \mathrm{J}\) of heat at constant volume and its temperature rises from \(27^{\circ} \mathrm{C}\) to \(37^{\circ} \mathrm{C}\). The value of \(\Delta U\) is

(a) \(100 \mathrm{~kJ}\)

(b) \(10 \mathrm{~kJ}\)

(c) 0

(d) \(1 \mathrm{~kJ}\).

44. The enthalpies of combustion of carbon and carbon monoxide are \(-\mathbf{3 9 3 . 5} \&\) \& \(-\mathbf{2 8 3 . 0} \mathrm{k.J} \mathrm{mol}^{-}\) ' respectively. The enthalpy of formation of carbon monoxide is

(a) \(-676.5 \mathrm{~kJ}\)

(b) \(110.5 \mathrm{~kJ}\)

(c) \(-110.5 \mathrm{~kJ}\)

(d) \(676.5 \mathrm{~kJ}\).

45. The standard enthalpies of formation of \(\mathrm{HCl}(\mathrm{g})\), \(\mathrm{H}(\mathrm{g})\) and \(\mathrm{Cl}(\mathrm{g})\) are \(-92.2,217.7\) and \(121.4 \mathrm{~kJ}\) \(\mathrm{mol}^{-1}\) respectively. The bond dissociation energy of \(\mathrm{HCl}\) is

(a) \(+431.3 \mathrm{~kJ}\)

(b) \(236.9 \mathrm{~kJ}\)

(c) \(-431.3 \mathrm{~kJ}\)

(d) \(339.1 \mathrm{~kJ}\).

46. Calculate the heat required to make \(6.4 \mathrm{~kg}\) of \(\mathrm{CaC}_2\) from \(\mathrm{CaO}\) (s) and \(\mathrm{C}\) (s) from the reaction \(\mathrm{CaO}(\mathrm{s})+3 \mathrm{C}(\mathrm{s}) \rightarrow \mathrm{CaC}_2(\mathrm{~s})+\mathrm{CO}(\mathrm{g})\) given that \(\Delta_j \mathrm{H}^0(\mathrm{CaO})=-151.6 \mathrm{kcal}, \Delta_J \mathrm{H}^0\left(\mathrm{CaC}_2\right)=-14.2\) kcal, \(\Delta \mathrm{H}^{\bullet}(\mathrm{CO})=-26.4\) kcal.

(a) \(5624 \mathrm{kcal}\)

(b) \(1.1 \times 10^4 \mathrm{kcal}\)

(c) \(86.24 \times 10^3\)

(d) \(1100 \mathrm{kcal}\).

47. Four grams of helium is expanded from 1 atm to one-tenth of its original pressure at \(30^{\circ} \mathrm{C}\). Change in entropy (assuming ideal gas behaviour) is

(a) \(38.3 \mathrm{JK}^{-1}\)

(b) \(76.6 \mathrm{JK}^{-1}\)

(c) \(19.15 \mathrm{JK}^{-1}\)

(d) \(100 \mathrm{JK}^{-1}\)

48. 48. For the reaction at \(300 \mathrm{~K}\)

$$

\begin{aligned}

& A(\mathrm{~g})+\mathrm{E}(\mathrm{g}) \rightarrow \mathrm{C}(\mathrm{g}) \\

& \Delta \mathrm{U}=-3.0 \mathrm{kcal} \Delta S=-10.0 \mathrm{cal} / \mathrm{K} \\

& \left(\mathrm{R}=2 \mathrm{cal} \mathrm{mol}^{-1} \mathrm{~K}^{-1}\right)

\end{aligned}

$$

\(\Delta \mathrm{G}\) is

(a) \(-600 \mathrm{cal}\)

(b) \(-3600 \mathrm{cal}\)

(c) \(2400 \mathrm{cal}\)

(d) \(3000 \mathrm{cal}\).

49. For the reaction, \(2 \mathrm{H}_2 \mathrm{O}(\mathrm{g}) \rightarrow 2 \mathrm{H}_2(\mathrm{~g})+\mathrm{O}_2(\mathrm{~g})\) \(\Delta_1 \mathrm{H}^0\) of water is

(a) \(285.8 \mathrm{~kJ}\)

(b) \(-285.8 \mathrm{~kJ}\)

(c) \(1143.2 \mathrm{~kJ}\)

(d) \(1243.2 \mathrm{~kJ}\).

50. If equilibrium constant \(K\) is \(10^3\), the \(\Delta G^{\bullet}\) for the reaction at \(300 \mathrm{~K}\) is (assume \(R=8 \mathrm{JK}^{-1}\) \(\mathbf{m o l}^{-1}\) )

(a) \(-16.582 \mathrm{~kJ}\)

(b) \(16.582 \mathrm{~kJ}\)

(c) \(165.82 \mathrm{~kJ}\)

(d) \(1658.2 \mathrm{~kJ}\).