The heat of combustion of carbon to CO₂ is -393.5 KJ/mol. The heat changed upon the formation of 35.2 g of CO₂ from carbon and oxygen gas is -
1. -315 KJ
2. +315 KJ
3. -630 KJ
4. +630 KJ

Which of the following statements is correct for a reversible process in a state of equilibrium?
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 statements is correct for the spontaneous adsorption of a gas ?

1. $∆$S is negative and therefore, $∆$H should be highly positive
2. $∆$S is negative and therefore, $∆$H should be highly negative
3. $∆$S is positive and therefore, $∆$H should be negative
4. $∆$S is positive and therefore, $∆$H should also be highly positive

Given the reaction : 
X₂O₄(l) → 2XO₂(g) 
ΔU = 2.1 kcal, ΔS = 20 cal K^–1 at 300 K 
The value of ΔG is:
1. 2.7 kcal
2. -2.7 kcal
3. 9.3 kcal
4. -9.3 kcal

In which of the following reactions, standard reaction entropy change $(∆S^0)$ is positive and standard Gibb's energy change $(∆G^0)$ decreases sharply with increasing temperature?

1. $C\left(graphite\right)+\frac{1}{2}{O}_2\left(g\right)\to CO\left(g\right)$

2. $CO\left(g\right)+\frac{1}{2}{O}_2\left(g\right)\to C{O}_2\left(g\right)$

3. $Mg\left(s\right)+\frac{1}{2}{O}_2\left(g\right)\to MgO\left(s\right)$

4. $\frac{1}{2}C\left(graphite\right)+\frac{1}{2}{O}_2\left(g\right)\to \frac{1}{2}C{O}_2\left(g\right)$

The enthalpy of fusion of water is 1.435 kcal/mol. The molar entropy change for the melting of ice at 0 ^oC is:

1. 10.52 cal/(mol K)

2. 21.04 cal/(mol K)

3. 5.260 cal/(mol K)

4. 0.526 cal/(mol K)

Standard enthalpy of vaporization ${∆}_{\mathrm{vap}}{\mathrm{H}}^0$for water at 100⁰C is 40.66 Kj mol^-1. The internal energy of vaporization of water at 100⁰C (in kJ mol^-1) is 
(Assume water vapour to behave like an ideal gas).

1. +37.56

1. -43.76

3. +43.76

4. +40.66

Which of the following is the correct option for free expansion of an ideal gas under adiabatic condition?
1.  $\mathrm{q}\ne 0, ∆\mathrm{T}=0, \mathrm{W}=0$
2.  $\mathrm{q}=0, ∆\mathrm{T}=0, \mathrm{W}=0$
3.  $\mathrm{q}=0, ∆\mathrm{T}<0, \mathrm{W}\ne 0$
4.  $\mathrm{q}=0, ∆\mathrm{T}\ne 0, \mathrm{W}=0$

Given the following reaction:
4H(g)→ 2H₂ (g) 
The enthalpy change for the reaction is -869.6 kJ. The dissociation energy of the H-H bond is -
1. -869.6 kJ
2. +434.8kJ
3. +217.4kJ
4. -434.8 kJ