Hydrolysis of sucrose is given by the following reaction:
$\text{Sucrose} + H_{2}O \rightleftharpoons \text{Glucose} + \text{Fructose}$
If the equilibrium constant $(K_{c})$ is $2 \times 10^{13}$ at $300 \ K$,the value of $\Delta_{r}G^{\Theta}$ at the same temperature will be:

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