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Hydrolysis of sucrose is given by the following reaction.
Sucrose \( +\mathrm{H}_{2} \mathrm{O} \rightleftharpoons \) Glucose \( + \) Fructose
If the equilibrium constant \( \left(K_{C}\right) \) is \( 2 \times 10^{13} \) at \( 300 \mathrm{~K} \), the value of \( \Delta_{r} G^{\ominus} \) at the same temperature will be:
[NEET 2020]
(a) \( 8.314 \mathrm{~J} \mathrm{~mol}^{-1} \mathrm{~K}^{-1} \times 300 \mathrm{~K} \times \ln \left(2 \times 10^{13}\right) \)
(b) \( 8.314 \mathrm{~J} \mathrm{~mol}^{-1} \mathrm{~K}^{-1} \times 300 \mathrm{~K} \times \ln \left(3 \times 10^{13}\right) \)
(c) \( -8.314 \mathrm{~J} \mathrm{~mol}^{-1} \mathrm{~K}^{-1} \times 300 \mathrm{~K} \times \ln \left(4 \times 10^{13}\right) \)
(d) \( -8.314 \mathrm{~J} \mathrm{~mol}^{-1} \mathrm{~K}^{-1} \times 300 \mathrm{~K} \times \ln \left(2 \times 10^{13}\right) \)
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