Problem: Consider the reaction at 298 K: 2 H2S(g) + SO2(g) → 3 S(s, rhombic) + 2 H2O(g) ΔG˚rxn = –102 kJIs the reaction more or less spontaneous under these conditions than under standard conditions?PH2S = 2.00 atm; PSO2 = 1.50 atm; PH2O = 0.0100 atm

FREE Expert Solution

Recall that ΔG and K are related to each other:

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

And the Kp expression for this reaction is:

2 H2S(g) + SO2(g) → 3 S(s, rhombic) + 2 H2O(g)

$\overline{){{\mathbf{K}}}_{{\mathbf{p}}}{\mathbf{=}}\frac{\mathbf{products}}{\mathbf{reactants}}{\mathbf{=}}\frac{\mathbf{\left(}{\mathbf{P}}_{{\mathbf{H}}_{\mathbf{2}}\mathbf{O}}{\mathbf{\right)}}^{\mathbf{2}}}{{\left({P}_{{H}_{2}S}\right)}^{\mathbf{2}}\left({P}_{{\mathrm{SO}}_{2}}\right)}}$

Problem Details

Consider the reaction at 298 K: 2 H2S(g) + SO2(g) → 3 S(s, rhombic) + 2 H2O(g) ΔG˚rxn = –102 kJ

Is the reaction more or less spontaneous under these conditions than under standard conditions?

PH2S = 2.00 atm; PSO2 = 1.50 atm; PH2O = 0.0100 atm