Calculate ΔG o for the following reaction at 25°C: 3Mg (s) + 2Al3 + (aq) ⇌ 3Mg2 + (aq) + 2Al (s) Enter your answer in scientific notation. * 10 kJ / mol

-3.7771 * 10² kJ/mol

Explanation:

Let's consider the following equation.

3 Mg (s) + 2 Al³⁺ (aq) ⇌ 3 Mg²⁺ (aq) + 2 Al (s)

We can calculate the standard Gibbs free energy (ΔG°) using the following expression.

ΔG° = ∑np. ΔG°f (p) - ∑nr. ΔG°f (r)

where,

n: moles

ΔG°f () : standard Gibbs free energy of formation

p: products

r: reactants

ΔG° = 3 mol * ΔG°f (Mg²⁺ (aq)) + 2 mol * ΔG°f (Al (s)) - 3 mol * ΔG°f (Mg (s)) - 2 mol * ΔG°f (Al³⁺ (aq))

ΔG° = 3 mol * (-456.35 kJ/mol) + 2 mol * 0 kJ/mol - 3 mol * 0 kJ/mol - 2 mol * (-495.67 kJ/mol)

ΔG° = - 377.71 kJ = - 3.7771 * 10² kJ

This is the standard Gibbs free energy per mole of reaction.