NEET UG 2020 — Chemistry Physical Chemistry

2020mcqhard

Hydrolysis of sucrose is given by the following reaction.

Sucrose $+{H}_{2}O\rightleftharpoons$ 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:

Official previous-year question

Held on 30 Apr 2020 · Verified 9 Jul 2026.

Options

A
$8.314 J{\mathrm{mol}}^{–1}{K}^{–1}\times 300 K\times \mathrm{ln}(2\times {10}^{13})$
B
$8.314 J{\mathrm{mol}}^{–1}{K}^{–1}\times 300 K\times \mathrm{ln}(3\times {10}^{13})$
C
$–8.314 J{\mathrm{mol}}^{–1}{K}^{–1}\times 300 K\times \mathrm{ln}(4\times {10}^{13})$
D
$–8.314 J{\mathrm{mol}}^{–1}{K}^{–1}\times 300 K\times \mathrm{ln}(2\times {10}^{13})$

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

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

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

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

NEET UG 2020 — Chemistry Physical Chemistry

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NEET UG 2020 — Chemistry Physical Chemistry

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NEET UG Physical Chemistry in other years

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