Metallic aluminum can react with water to create aluminum oxide and hydrogen gas as shown in the equation $2 Al (s) + 3 H_{2} O (g) ? Al_{2} O_{3} (s) + 3 H_{2} (g)$ Given the free energy changes of formation in the table, calculate the standard free energy change, $? G^{?}$ , for the reaction. $186 kJ / mol$ $? 891 kJ / mol$ $? 91.6 kJ / mol$ $? 223 kJ / mol$

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Metallic aluminum can react with water to create aluminum oxide and hydrogen gas as shown in the equation

2 Al (s) + 3 H_{2} O (g) ? Al_{2} O_{3} (s) + 3 H_{2} (g)

Given the free energy changes of formation in the table, calculate the standard free energy change,

? G^{?}

, for the reaction.

186 kJ / mol

? 891 kJ / mol

? 91.6 kJ / mol

? 223 kJ / mol

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