Question

Hydrolysis of sucrose is given by the following reaction.$\text{Sucrose}+H_{2}O\rightleftharpoons \text{Glucose + Fructose}$
If the equilibrium constant $\left(K_C\right)$ is $2\times {10}^{13}\text{at}300K$, The value of ${\Delta }_r{G}^{\circ }$ at the same temparature will be :

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

Answer 1

The correct option is B $-8.314J{\text{mol}}^{-1}{K}^{-1}\times 300K\times ln(2\times {10}^{13})$

$\Delta G^{\circ }=-RTlnK$$\Rightarrow -8.314J{\text{mol}}^{-1}{K}^{-1}\times 300K\times ln(2\times {10}^{13})$