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

Match the statements given in column 1 with corresponding characteristics given in column II and choose the correct option:

Codes:

 For conversion of oxygen to ozone, $\frac{3}{2}{\mathrm{O}}_2\left(\mathrm{g}\right)\to {\mathrm{O}}_3\left(\mathrm{g}\right)$ at 298 K, the value of Kp for this conversion is 2.47 × 10^–29. The value of  ∆_rG^⊖ is-

Consider the following reaction at 298 K

$2N{H}_3\left(g\right) + C{O}_2\left(g\right) \leftrightharpoons N{H}_{2}CON{H}_2\left(aq\right) + H_{2}O\left(l\right)$

For the above reaction, the standard Gibbs energy change, ∆_rG^⊖ at the given temperature is –13.6 kJ mol^–1. The value of equilibrium constant is:

1. 6.4 × 10⁵

2. 2.4 × 10²

3. 4.4 × 10²

4. 4.4 × 10⁵

At 60°C, dinitrogen tetroxide is 50 percent dissociated. The standard free energy change at this temperature will be:
1. -863.8   kJmol^-1
2.  -652.7  kJmol^-1
3. -763.8 kJmol^-1 
4.  -789.9   kJmol^-1

Hydrolysis of sucrose is given by the following reaction

Sucrose + H₂O $\rightleftharpoons$ Glucose + Fructose

If the equilibrium constant (K_c) is 2$\times$10¹³ at 300 K, the value of ${∆}_r{G}^{⊝}$ at the same temperature will be:

1. 8.314 J mol^–1 K^–1$\times$300 K$\times$ln (2$\times$10¹³)

2. 8.314 J mol^–1 K^–1$\times$300 K$\times$ln (3$\times$10¹³)

3. –8.314 J mol^–1 K^–1$\times$300 K$\times$ln (4$\times$10¹³)

4. –8.314 J mol^–1 K^–1$\times$300 K$\times$ln (2$\times$10¹³)