Q. Hydrolysis of sucrose is given by the following reaction. Sucrose + $H_2O \rightleftharpoons$ Glucose + Fructose If the equilibrium constant ($K_c$) is $2 \times 10^{13}$ at 300 K, the value of $\Delta_rG^\circ$ at the same temperature will be :
A) 8.314 J $mol^{-1}K^{-1}$ × 300 K × ln($2 \times 10^{13}$)
B) 8.314 J $mol^{-1}K^{-1}$ × 300 K × ln($3 \times 10^{13}$)
C) -8.314 J $mol^{-1}K^{-1}$ × 300 K × ln($4 \times 10^{13}$)
D) -8.314 J $mol^{-1}K^{-1}$ × 300 K × ln($2 \times 10^{13}$)
Explanation
[Solution] $\Delta_rG^\circ = -RT\ln K_c = -8.314 \times 300 \times \ln(2 \times 10^{13})$. Answer (4).
Reviewed by Dr. Abubacker
Physics Educator & NEET/JEE Specialist
Ph.D. in Physics with 19+ years of teaching experience.