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

Question

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]

Smart Achievers · Accepted Answer

(37)

$Δ G ° = Δ H ° - T Δ S °$

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

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

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

$- 2.303 RT \log_{10} K = ΔG °$

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

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

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

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]

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Solution

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

Ans. (37) ΔG°=ΔH°-TΔS° ΔG°=77.2 kJ mol-1-400 K×122 JK-1 =77.2×1000 Jmol-1-400 K×122 JK-1 =28400 J mol-1 -2.303 RT log10K=ΔG° -2.303 RT log10Keq=28400 Jmol-1 -2.303×8.314 Jmol-1 K-1×400 K×log10Keq=28400 Jmol-1 log10Keq=-3.7=-37×10-1

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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]