Hydrolysis of sucrose is given by the following reaction:
$$\text{Sucrose}+{\text{H}}_2\text{O}\rightleftharpoons \text{Glucose}+\text{Fructose}$$
If the equilibrium constant ($K_c$) is $2\times 10^{13}$ at $300\text{K}$, the value of ${\Delta }_r{G}^{\circ }$ at the same temperature will be:

1. A
   $-8.314{\text{J mol}}^{-1}{\text{K}}^{-1}\times 300\text{K}\times \ln (2\times 10^{13})$
2. B
   $8.314{\text{J mol}}^{-1}{\text{K}}^{-1}\times 300\text{K}\times \ln (2\times 10^{13})$
3. C
   $8.314{\text{J mol}}^{-1}{\text{K}}^{-1}\times 300\text{K}\times \ln (3\times 10^{13})$
4. D
   $-8.314{\text{J mol}}^{-1}{\text{K}}^{-1}\times 300\text{K}\times \ln (4\times 10^{13})$