The value of log K for the reaction A B at 298 K is _______. (Nearest integer) Given: H = - 54.07?kJ mol - 1 S = 10?J K - 1 mol - 1 (Take 2.303×8.314×298=5705) [2023]

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Solution

Q.
The value of log K for the reaction $A ⇌ B$ at 298 K is _______. (Nearest integer)

$Given: Δ H ° = - {54.07 kJ mol}^{- 1}$

$Δ S ° = {10 J K}^{- 1} {mol}^{- 1}$

$(Take 2.303×8.314×298=5705)$ [2023]

Ans.
(10)

$Δ G ° = Δ H ° - T Δ S °$

$Δ G ° = - 54070 - 298 \times 10 = - 57050 J$

$Δ G ° = - {2.303 RT log K}_{e q}$

$- 57050 J = - {5705 log K}_{e q}$

${log K}_{e q} = 10$

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