Calculate ΔGo (in kJ/mol) for the following reaction at 1 atm and 25∘C: C2H6(g) + O2(g) → CO2(g)+ H2O (l) ΔGf∘ C2H6(g) = -32.89 kJ/mol; ΔGf∘ CO2(g) = -394.4 kJ/mol; ΔGf∘ H2O (l) = -237.2 kJ/mol
To find: ΔGo ?
Given: ΔGf∘ C2H6(g) = -32.89 kJ/mol; ΔGf∘ CO2(g) = -394.4 kJ/mol; ΔGf∘ H2O (l) = -237.2 kJ/mol
Step 1. Since gibbs free energy of product = gibbs free of reactant thus,
= ΔGf∘ CO2(g) + ΔGf∘ H2O (l) = ΔGf∘ C2H6(g) + ΔGo
= -394.4 - 237.2 = -32.89 + ΔGo
Thus, value of ΔGo = -598.71 KJ/mol
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