From the following bond energies:
H—H bond energy: 431.37 kJ mol^-1 
C=C bond energy: 606.10 kJ mol^-1 
C—C bond energy: 336.49 kJ mol^-1 
C—H bond energy: 410.50 kJ mol^-1 
Enthalpy for the reaction, 

will be:

1.	1523.6 kJ mol-1	2.	-243.6 kJ mol-1
3.	-120.0 kJ mol-1	4.	553.0 kJ mol-1

The values of ΔH and ΔS for the given reaction are 170 kJ and 170 JK^-1, respectively.
C_(graphite) + CO₂(g)→2CO(g) 
This reaction will be spontaneous at:

1. 710 K
2. 910 K
3. 1110 K
4. 510 K

The correct statement for a reversible process in a state of equilibrium is:
1. $∆$G = – 2.30RT log K
2. $∆$G = 2.30RT log K
3. $∆$G^o = – 2.30RT log K
4. $∆$G^o = 2.30RT log K

Which of the following is correct for isothermal expansion of an ideal gas -

1. W_rev = W_irr

2. W_rev + W_irr = 0

3. W_rev > W_irr

4. q_rev = q_irr

Which, among the following, is not a state function?

1. Internal energy

2. Free energy

3. Work

4. Enthalpy

Which among the following state functions is an extensive property of the system?

The bond energies of $\mathrm{C}\equiv \mathrm{C}$, C-H, H-H, and C=C are 198, 98, 103 and145 kcal respectively.

The enthalpy change of the reaction $\mathrm{HC}\equiv \mathrm{CH}+{\mathrm{H}}_2\to {\mathrm{C}}_2{\mathrm{H}}_4$ would be-

1. 48 kcal

2. 96 kcal

3. -40 kcal

4. -152 kcal

As an isolated box, equally partitioned, contains two ideal gasses A and B as shown:

When the partition is removed, the gases mix. The changes in enthalpy $(∆\mathrm{H})$ and entropy $(∆\mathrm{S})$ in the process, respectively, are

1. Zero, positive

2. Zero, negative

3. Positive, zero

4. Negative, zero

The entropy change in the isothermal reversible expansion of 2 moles of an ideal gas from 10 to 100 L at 300 K is

1. $42.3 \mathrm{J} {\mathrm{K}}^{-1}$

2. $35.8 \mathrm{J} {\mathrm{K}}^{-1}$

3. $38.3 \mathrm{J} {\mathrm{K}}^{-1}$

4. $32.3 \mathrm{J} {\mathrm{K}}^{-1}$