We’re being asked to calculate AG° (in kJ/mol) for the following reaction at 1 atm and 25°C:

C_{2}H_{6}(g) + O_{2}(g) → CO_{2}(g) + H_{2}O(l)

We can use the following equation to solve for ** ΔG˚_{rxn}**:

$\overline{){\mathbf{\Delta G}}{{\mathbf{\xb0}}}_{{\mathbf{rxn}}}{\mathbf{=}}{\mathbf{\Delta G}}{{\mathbf{\xb0}}}_{\mathbf{f}\mathbf{,}\mathbf{}\mathbf{prod}}{\mathbf{-}}{\mathbf{\Delta G}}{{\mathbf{\xb0}}}_{\mathbf{f}\mathbf{,}\mathbf{}\mathbf{react}}}$

Calculate ΔG° (in kJ/mol) for the following reaction at 1 atm and 25°C:

C_{2}H_{6} (g) + O_{2} (g) → CO_{2} (g) + H_{2}O (l)

ΔG_{f }°C_{2}H_{6} (g) = 32.89 kJ/mol

ΔG_{f}°_{ }CO_{2 }(g) = 394.4 kJ/mol

ΔG_{f}°_{ }H_{2}O (l) = 237.2 kJ/mol

Frequently Asked Questions

What scientific concept do you need to know in order to solve this problem?

Our tutors have indicated that to solve this problem you will need to apply the Gibbs Free Energy concept. You can view video lessons to learn Gibbs Free Energy. Or if you need more Gibbs Free Energy practice, you can also practice Gibbs Free Energy practice problems.