Calculate the Gibbs Free Energy G for a reactio... - SS2 Chemistry Chemical Thermodynamics Question
Calculate the Gibbs Free Energy (ΔG) for a reaction given the following information:
Reaction: 2H2O(g) → 2H2(g) + O2(g)
ΔGf° (H2O(g)): -237.2 kJ/mol
ΔGf° (H2(g)): 0 kJ/mol
ΔGf° (O2(g)): 0 kJ/mol
ΔG = 2 × ΔGf° (H2(g)) + ΔGf° (O2(g)) - 2 × ΔGf° (H2O(g))
= 2 × 0 kJ/mol + 0 kJ/mol - 2 × (-237.2 kJ/mol)
= 474.4 kJ/mol
Please note that the ΔHf°, ΔS°, and ΔGf° values used in these calculations represent the standard enthalpy, entropy, and Gibbs free energy of formation, respectively, at 25°C (298 K) and 1 atm pressure.
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