Hydrolysis of sucrose is given by the following reaction.
Sucrose $+{\mathrm{H}}_2\mathrm{O}\rightleftharpoons$ Glucose $+$ Fructose
If the equilibrium constant $\left({\mathrm{K}}_{\mathrm{C}}\right)$ is $2\times {10}^{13}$ at $300\mathrm{K}$, the value of ${\mathrm{\Delta }}_{\mathrm{r}}{\mathrm{G}}^{\ominus }$ at the same temperature will be:

• A

  $8.314\mathrm{J} {\mathrm{mol}}^{–1}{\mathrm{K}}^{–1}\times 300\mathrm{K}\times \ln \left(2\times {10}^{13}\right)$
• B

  $8.314\mathrm{J} {\mathrm{mol}}^{–1}{\mathrm{K}}^{–1}\times 300\mathrm{K}\times \ln \left(3\times {10}^{13}\right)$
• C

  $–8.314\mathrm{J} {\mathrm{mol}}^{–1}{\mathrm{K}}^{–1}\times 300\mathrm{K}\times \ln \left(4\times {10}^{13}\right)$
• Correct answer
  D

  $–8.314\mathrm{J} {\mathrm{mol}}^{–1}{\mathrm{K}}^{–1}\times 300\mathrm{K}\times \ln \left(2\times {10}^{13}\right)$

Hence, the correct answer is option: 'D'.