The value of \log_{10} K for a reaction A ⇌ B is (Given: \Delta_r H_{298 K} = – 54.07 kJ mol^{–1} and \Delta_r S = 10 JK^{−1}mol^{−1} R = 8.314 J K^{−1}mol^{−1} ; 2.303 × 8.314 × 298 = 5705) [JEE Adv 2007 P1]

IIT JEE Advanced 2007 Paper 1

Section: Chemistry

Question : 31 of 66

Marks: +1, -0

The value of log10 K for a reaction A ⇌ B is
(Given: ΔrH298K = – 54.07 kJmol–1 and ΔrS = 10 JK−1mol−1
R = 8.314 JK−1mol−1 ; 2.303 × 8.314 × 298 = 5705)

[JEE Adv 2007 P1]

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