Solved: Chemistry Question for NEET

NEET ChemistryMedium

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 $\Delta_r G^{\ominus}$ at the same temperature will be :

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

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

$8.314 \text{ J mol}^{-1} \text{K}^{-1} \times 300 \text{ K} \times \ln(3 \times 10^{13})$

$-8.314 \text{ J mol}^{-1} \text{K}^{-1} \times 300 \text{ K} \times \ln(4 \times 10^{13})$

Step-by-Step Solution

$\Delta G = \Delta G^{\ominus} + RT \ln Q$ . At equilibrium $\Delta G = 0, Q = K_{eq}$ . So $\Delta_r G^{\ominus} = -RT \ln K_{eq}$ . $\Delta_r G^{\ominus} = -8.314 \text{ J mol}^{-1} \text{K}^{-1} \times 300 \text{ K} \times \ln(2 \times 10^{13})$ .

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