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

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

Standard entropies of X₂, Y₂ and XY₃ are 60, 40 and 50JK^-1mol^-1 respectively. For the reaction 
$\frac{1}{2}{\mathrm{X}}_2 + \frac{3}{2}{\mathrm{Y}}_2 \leftrightharpoons {\mathrm{XY}}_3 ; ∆\mathrm{H} = -30 \mathrm{kJ}$ to  be at equilibrium, the temperature should be

1. 750 K

2. 1000 K

3. 1250 K

4. 500 K

For vaporization of water at 1 atmospheric pressure, the values of ∆H and ∆S are 40.63 kJ mol^–1 and 108.8 JK^–1 mol^–1, respectively. The temperature when Gibbs energy change (∆G) for this transformation will be zero, is -

1. 393.4 K

2. 373.4 K

3. 293.4 K

4. 273.4 K

Match List – I (Equations) with List – II (Type of processes) and select the correct option.

    List –I                                    List – II
    Equation                             Type of processes

(a) K_p > Q                           (i) Non spontaneous
(b) ∆G^º < RT ln Q                 (ii) Equilibrium
(c) K_p = Q                           (iii) Spontaneous and endothermic
(d) T > $\frac{∆H}{∆S}$                       (iv) Spontaneous

Options :
      (a)  (b)  (c)   (d)
1. (iii)  (iv)  (ii)   (i)
2. (iv)   (i)   (ii)   (iii)
3. (ii)    (i)   (iv)  (iii)
4. (i)    (ii)   (iii)  (iv)

The values of ΔH and ΔS for the reaction, C_(graphite) + CO₂(g)→2CO(g) are 170 kJ and 170 JK^-1, respectively. This reaction will be spontaneous at
1. 710 K
2. 910 K
3. 1110 K
4. 510 K

1.  (I) and (IV)

2.  (II), (III) and (IV)

3.  (I), (II) and (III)

4.  (II) and (III)