Please be patient as the PDF generation may take up to a minute.

1. Identify which of the following is the correct option for free expansion of an ideal gas under adiabatic condition.
1. \(\Delta \mathrm{q} \neq 0, \Delta \mathrm{~T}=0, \mathrm{~W}=0 \)
2. \(\Delta \mathrm{q}=0, \Delta \mathrm{~T}=0, \mathrm{~W}=0 \)
3. \(\Delta \mathrm{q}=0, \Delta \mathrm{~T}<0, \mathrm{~W} \neq 0 \)
4. \(\Delta \mathrm{q}=0, \Delta \mathrm{~T} \neq 0, \mathrm{~W}=0\)

2.

Consider the given reaction:
\(C H_{3} C O O H \left(\right. l \left.\right)+ 2 O_{2} \left(\right. g \left.\right) \rightleftharpoons 2 C O_{2} \left(\right. g \left.\right)+ 2 H_{2} O \left(\right. l \left.\right)\)
At 25°C and 1 atm. pressure, ΔH = –874 kJ. The change in internal energy (ΔE) is:
1. – 874 kJ
2. – 971.53 kJ
3. + 971.53 kJ
4. + 874 kJ

3.

Which of the following are not state functions?
I. q + w
II. q 
III. w
IV. H - TS
1. I, II & III
2. II & III
3. I & IV
4. II, III & IV

4. 1 mole of gas undergoes an adiabatic process, given that:
\(C_v=20 \ \mathrm{JKmol}^{-1}, W=3 \ \mathrm{kJ}, \ T_1=27 \ ^ {\circ} \mathrm{C} \) 
What is the value of \(T_2\)​ in ^oC?
1. 169 
2. 184
3. 177 
4. 191

5. Given below are two statements: 

Statement I	A process or change is said to be reversible if it is brought out in such a way that the process can, at any point, be reversed by an infinitesimal change.
Statement II	A reversible process proceeds infinitely slowly through a series of equilibrium states such that the system and its surroundings are always in near equilibrium with each other.

 

1.	Both statement I and statement II are correct.
2.	Both statement I and statement II are incorrect.
3.	Statement I is correct but statement II is incorrect.
4.	Statement I is incorrect and statement II is correct.

6. Determine \(\Delta U\) for the process where, one mole of an ideal gas at 300 K is expanded isothermally from 1 L to 10 L volume:
(Use R = 8.314 J K^–1 mol^–1)

1.	1260 J	2.	2520 J
3.	5040 J	4.	0 J

7. Calculate the magnitude of heat (q) in joules for an isothermal irreversible expansion, where the system expands against an external pressure of 8 bar, and the volume increases by 10 L.

1.	8000 J	2.	2000 J
3.	6000 J	4.	7600 J

8. Match Column I (Reactions) with Column II (Enthalpy) and mark the appropriate choice:
 

	Column I (Reactions)		Column II (Enthalpy)
(A)	\(\small{CH_{4(g)} + 2O_{2(g)} \rightarrow CO_{2(g)} + 2H_2O}\)	(i)	\(\Delta _{sol}H^o\)
(B)	\( H_{2(g)} \rightarrow 2H_{(g)}\)	(ii)	\(\Delta _{lattice}H^o\)
(C)	\(NaCl_{(s)} \rightarrow Na^+_{(g)} + Cl^-_{(g)} \)	(iii)	\(\Delta _{c}H^o\)
(D)	\(NaCl_{(s)} \rightarrow Na^+_{(aq)} + Cl^-_{(aq)} \)	(iv)	\(\Delta _{bond}H^o\)

1. (A) →(iv), (B)→(iii), (C) →(i), (D)→ (ii)
2. (A) →(ii), (B)→(i), (C) →(iv), (D)→ (iii)
3. (A) →(i), (B)→(ii), (C) →(iii), (D)→ (iv)
4. (A) →(iii), (B)→(iv), (C) →(ii), (D)→ (i)

9. Which of the following is the maximum energy available for useful work from a spontaneous reaction?

1.	Gibbs free energy	2.	Lattice energy
3.	Kinetic energy	4.	Ionization energy

10. Given the following reaction:
\(\begin{aligned} & \frac{1}{2} \mathrm{H}_2+\frac{1}{2} \mathrm{Cl}_2 \rightarrow \mathrm{HCl} \\ & \Delta H_f(\mathrm{HCl})=-93 \mathrm{~kJ} / \mathrm{mol} \\ & \text { B.E }\left(\mathrm{H}_2\right)=434 \mathrm{~kJ} / \mathrm{mol}, \text { B.E }\left(\mathrm{Cl}_2\right)=242 \mathrm{~kJ} / \mathrm{mol} \end{aligned}\)
The bond dissociation energy of HCl in the above reaction will be:
1. 232 kJ/mol
2. 331 kJ/mol
3. 431 kJ/mol
4. 530 kJ/mol