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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 $\Delta_r G^0$ at the same temperature will be:

medium

Thermodynamics

2020

chemistry

$8.314 \times 300 \times \ln(2 \times 10^{13})$

$8.314 \times 300 \times \ln(3 \times 10^{13})$

Explanation

To solve this problem, we need to calculate the standard Gibbs free energy change $\Delta_r G^0$ using the relation between $K_c$ and $\Delta_r G^0. \\$

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Hydrolysis of sucrose is given by the following reaction: \\ Sucrose+H2O⇌ + H_2O \rightleftharpoons +H2​O⇌Glucose+ + +Fructose \\ If the equilibrium constant Kc K_c Kc​ is 2×1013 2 \times 10^{13} 2×1013 at 300 K, the value of ΔrG0 \Delta_r G^0 Δr​G0 at the same temperature will be:

Explanation

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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 $\Delta_r G^0$ at the same temperature will be: