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Hydrolysis of sucrose is given by the following reaction. Sucrose \( +\mathrm{H}_{2} \mathrm{O} \rightleftharpoons \) Gl…

Q1

Hydrolysis of sucrose is given by the following reaction.

Sucrose \( +\mathrm{H}_{2} \mathrm{O} \rightleftharpoons \) Glucose \( + \) Fructose

If the equilibrium constant \( \left(\mathrm{K}_{\mathrm{c}}\right) \) is \( 2 \times 10^{13} \) at \( 300 \mathrm{~K} \), the value of \( \Delta_{r} \mathrm{G}^{\mathrm{o}} \) 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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