Question

Hydrolysis of sucrose is given by the following reaction.
$Sucrose + H_20 \rightleftharpoons Glucose + Fructose$
If the equilibrium constant $(K_c)$ is $2 \times 10^{13}$ at 300K, the value of $\Delta_r$ $G^\ominus$ at the same temperature will be :

• A. $-8.314\, Jmol^{-1}K^{-1} \times 300 K \times ln (2\times10^{13})$
• B. $8.314 \,mol^{-1}K^{-1} \times 300 K \times ln (2 \times 10^{13})$
• C. $8.314 \, J \,mol^{-1} 300 K \times ln(3 \times 10^{13})$
• D. $-8.314 \,J\,mol^{-1} K^{-1} \times 300 \,K \times In(4 \times 10^{13})$

Answer 1

Answer: (A)

$-8.314\, Jmol^{-1}K^{-1} \times 300 K \times ln (2\times10^{13})$

Answer 2

$\Delta G^{\circ} = -RT\,ln\,K_C$
$\Delta G^{\circ} = -8.314 \times 300 \,ln ( 2 \times 10^{13})$