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1. The temperature at which the given reaction is in equilibrium is:
\(\mathrm{X_{(g)} +3Y_{(g)} \rightleftharpoons 2Z_{(g)} ; \Delta H= -40~ kJ ~mol^{-1}}~\)
(The standard entropies of X, Y, and Z are 60, 40, and 50 J K^–1 mol^–1, respectively.) 
1. 273 K 
2. 600 K 
3. 500 K 
4. 400 K 

2.

Which one of the following reactions obeys  ∆H ≠ ∆E?

1.	H 2 (g) + I 2 (g)  ⇌   2 HI (g)
2.	HCl (aq)   + NaOH (aq)→ NaCl (aq) + H2O (l)
3.	C (s) + O2 (g)   ⇌   CO2 (g)
4.	N2 (g) + 3H2 (g) → 2NH3 (g)

3. Match the items given in Column I with those given in Column II:

	Column I		Column II
A.	Temperature	i.	Path function
B.	Free energy	ii.	State function
C.	Heat
D.	Work

 

Options	(A)	(B)	(C)	(D)
1.	i	ii	ii	i
2.	ii	ii	i	i
3.	i	i	ii	i
4.	ii	ii	ii	i

4.

Which of the following options correctly represents the relationship between \(C_p \text { and } C_V\) for one mole of an ideal gas?

1.	\(C_P=R C_V \)	2.	\(C_V=RC_P \)
3.	\(C_P+C_V=R \)	4.	\(C_{{P}}-{C}_{{V}}={R}\)

5.

Assertion (A)	Absolute values of the internal energy of substances cannot be determined.
Reason (R)	It is impossible to determine the exact values of constituent energies of the substances.

 

1.	Both (A) and (R) are True and (R) is the correct explanation of (A).
2.	Both (A) and (R) are True but (R) is not the correct explanation of (A).
3.	(A) is True but (R) is False.
4.	Both (A) and (R) are False.

6. The enthalpy of a system increases by 50 kJ when its internal energy is increased by 113 kJ. What is the pressure in kNm^-2 of the system if the volume of gas is reduced by 10 m³ at constant pressure? 
[Given: 1 J = 1Nm]
1. 16.13
2. 6.30
3. 5.00 
4. 30.30

7.

Five moles of an ideal gas at 1 bar and 298 K undergo free expansion (expansion into vacuum) such that its volume becomes double. Calculate the work done during the process:

1. \( \mathrm{C}_{\mathrm{V}}\left(\mathrm{T}_2-\mathrm{T}_1\right)\)
2. \( \text {-RT }\left(\mathrm{V}_2-\mathrm{V}_1\right) \)
3. \( \text {-RT } \ln \mathrm({V}_1 / \mathrm{V}_2 )\)
4. Zero

8. What is the enthalpy change (ΔH) for the following reaction?
\(\mathrm {H}_2 \mathrm{C} = \mathrm {CH}_2 \text {(g)}+\mathrm{H}_2 \text {(g)} \rightarrow\mathrm {H}_3 \mathrm {C} - \mathrm {CH}_3 \text {(g)}\)
(Use the following bond energy data:
H-C: 413 kJ/mole 
H-H: 436 kJ/mole 
C=C: 614 kJ/mole 
C-C: 348 kJ/ mole )
1. -656 kJ/mole
2. -343 kJ/mole
3. -289 kJ/mole
4. -124 kJ/mole

9. For a given chemical reaction A ⇌ B at \(\text 300 ~ \text K\), the free energy change is \(– 49.4~\mathrm{kJ ~mol^{–1}}\) and the enthalpy of reaction is \(51.4~\mathrm{kJ~ mol^{–1} }\). The entropy change of the reaction is:  
1. \(140 ~\mathrm{JK^{–1} mol^{–1}}\)
2. \(671~\mathrm{JK^{–1} mol^{–1}}\)
3. \(336~\mathrm{JK^{–1} mol^{–1}}\)
4. \(390 ~\mathrm{JK^{–1} mol^{–1}}\)

10. What is the entropy change for the vaporization of water, if the molar heat of vaporization of water is \( +43.9~\text{kJ}\ mol^{-1}\) ?
1. \(8.49 \mathrm{~J} \mathrm{~mol}^{-1} \mathrm{~K}^{-1}\)
2. \(4.184 \mathrm{~J} \mathrm{~mol}^{-1} \mathrm{~K}^{-1}\)
3. \(2.78 \mathrm{~J} \mathrm{~mol}^{-1} \mathrm{~K}^{-1}\)
4. \(118 \mathrm{~J} \mathrm{~mol}^{-1} \mathrm{~K}^{-1}\)