Calculate Δ_rG° for the reaction below at 25.0 °C. CH₄(g) + H₂O(g) → 3 H₂(g) + CO(g)
Given: Δ_fG° [CH₄(g) ] = -50.8 kJ/mol,Δ_fG° [H₂O(g) ] = -228.6 kJ/mol,Δ_fG° [H₂(g) ] = 0.0 kJ/mol,and Δ_fG° [CO(g) ] = -137.2 kJ/mol.

Question

Quizplus · Accepted Answer

Δ_rG° = ΣnΔ_fG°(products) - ΣnΔ_fG°(reactants) First, we need to balance the equation: CH₄(g) + 4 H₂O(g) → 3 H₂(g) + CO(g) Δ_rG° = (3 mol x 0.0 kJ/mol) + (1 mol x (-137.2 kJ/mol)) - (1 mol x (-50.8 kJ/mol)) - (4 mol x (-228.6 kJ/mol)) Δ_rG° = +142.2 kJ/mol-rxn Therefore, the best choice is C. The positive value for Δ_rG° indicates that the reaction is not spontaneous at 25.0 °C.

Calculate ΔrG° for the Reaction Below at 25

Calculate Δ_rG° for the Reaction Below at 25