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NEET ChemistryGeneralMedium

Question

Hydrolysis of sucrose is given by the following reaction. Sucrose + H2O⇌H_2O \rightleftharpoons Glucose + Fructose. If the equilibrium constant (KcK_c) is 2×10132 \times 10^{13} at 300 K, the value of ΔrG⊖\Delta_r G^{\ominus} at the same temperature will be :

1

−8.314 J mol−1K−1×300 K×ln⁡(2×1013)-8.314 \text{ J mol}^{-1} \text{K}^{-1} \times 300 \text{ K} \times \ln(2 \times 10^{13})

2

8.314 J mol−1K−1×300 K×ln⁡(2×1013)8.314 \text{ J mol}^{-1} \text{K}^{-1} \times 300 \text{ K} \times \ln(2 \times 10^{13})

3

8.314 J mol−1K−1×300 K×ln⁡(3×1013)8.314 \text{ J mol}^{-1} \text{K}^{-1} \times 300 \text{ K} \times \ln(3 \times 10^{13})

4

−8.314 J mol−1K−1×300 K×ln⁡(4×1013)-8.314 \text{ J mol}^{-1} \text{K}^{-1} \times 300 \text{ K} \times \ln(4 \times 10^{13})

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