# Problem: Use data from appendix iib in the textbook to calculate the equilibrium constants at 25°C for each of the following reaction:2 H2S (g) ⇌ 2 H2(g) + S2(g)

###### FREE Expert Solution

2 H2S (g) ⇌ 2 H2(g) + S2(g)

$\overline{){\mathbf{\Delta G}}{{\mathbf{°}}}_{{\mathbf{rxn}}}{\mathbf{=}}{\mathbf{-}}{\mathbf{RTlnK}}}$

The values for ΔG˚f can be looked up in textbooks or online:

ΔG˚f, H2S(g) = –33.4 kJ/mol

ΔG˚f, H2(g) = 0 kJ/mol

ΔG˚f, S2(s) = 78.7 kJ/mol

Solving for ΔG˚rxn:

ΔG˚rxn145.5 kJ/mol

ΔG˚rxn145500 J/mol

We can now solve for the equilibrium constant using these given values:

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###### Problem Details

Use data from appendix iib in the textbook to calculate the equilibrium constants at 25°C for each of the following reaction:

2 H2S (g) ⇌ 2 H2(g) + S2(g)