Question

Hydrolysis of sucrose gives, $\text{Sucrose}+{\text{H}}_2\text{O}\rightleftharpoons \text{Glucose}+\text{Fructose}$

Equilibrium constant $K_c$ for the reaction is $2\times {10}^{13}$ at $300K$. Calculate $\Delta G^{\circ }$ at $300K$.

Answer 1

$\Delta G^{\circ }$ value

Given, $K_c=2\times {10}^{13},T=300K$

We know that $\Delta G^{\circ }$ and $K_c$ are related as-

$\Delta G^{\circ }=-RT\ln K_c$

Putting values in above equation we get:

$\Delta G^{\circ }=-8.314Jmo{l}^{-1}{K}^{–1}\times 300K\times \ln (2\times {10}^{13})$

$\Rightarrow \Delta G^{\circ }=-7.64\times {10}^{4}Jmo{l}^{–1}$