For a certain thermochemical reaction at ,log equilibrium constant (logk) is

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Solution

Q.
For a certain thermochemical reaction $M \to N$ at $T = 400 K$ , ${ΔH}^{⊝} = 77.2 kJ$ ${mol}^{- 1}, ΔS = 122 {JK}^{- 1}$ , log equilibrium constant (logk) is - ______ $\times 10^{- 1} .$ [2024]

Ans.
(37)

$Δ G ° = Δ H ° - T Δ S °$

$Δ G ° = 77.2 kJ {mol}^{- 1} - 400 K \times 122 {JK}^{- 1}$

$= 77.2 \times 1000 {Jmol}^{- 1} - 400 K \times 122 {JK}^{- 1}$

$= 28400 J {mol}^{- 1}$

$- 2.303 RT \log_{10} K = ΔG °$

$- 2.303 RT \log_{10} K_{eq} = 28400 J {mol}^{- 1}$

$- 2.303 \times 8.314 J {mol}^{- 1} K^{- 1} \times 400 K \times \log_{10} K_{eq} = 28400 J {mol}^{- 1}$

$\log_{10} K_{e q} = - 3.7 = - 37 \times 10^{- 1}$

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