The value of \log _{10} K for a reaction {\A} ⇋ {\B} is (Given : \\Delta_{{\r}} {\H^\circ}_{298 {\K}}=-54.07 {\kJ} {\mol}^{-1}, \\Delta_{{\r}} {\S^\circ}_{298 {\K}}=10 {\JK}^{-1} {\mol}^{-1} and {\R}=8.314 {\JK}^{-1} {\mol}^{-1}; (2.303 \times8.314 \times 298=5705 )

VITEEE 2021 Paper

Section: Chemistry

Question : 48 of 80

Marks: +1, -0

The value of log10K for a reaction A⇋B is
(Given : ΔrH°298K=−54.07‌kJ‌mol−1,
ΔrS°298K=10JK−1mol−1 and R=8.314JK−1 mol−1;
(2.303×8.314×298=5705 )

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