The reaction $2 "Mg"(s) + "O"_2(g) -> 2 "MgO"(s)$ has a free energy $DeltaG_"rxn" = -"597 kJ/mol"$ under standard conditions. What is the free energy of formation of $"MgO"$ ?

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The reaction $2 "Mg"(s) + "O"_2(g) -> 2 "MgO"(s)$ has a free energy $DeltaG_"rxn" = -"597 kJ/mol"$ under standard conditions. What is the free energy of formation of $"MgO"$ ?

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Answer 1 · 2016-11-16T12:39:17

-298.5 kJ/mol

Explanation:

-298.5 kJ/mol
The given reaction provides the Gibbs free energy of formation for the formation of two moles of MgO. Therefore, the $G_f$ for one mole is half that amount.

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The reaction $2 "Mg"(s) + "O"_2(g) -> 2 "MgO"(s)$ has a free energy $DeltaG_"rxn" = -"597 kJ/mol"$ under standard conditions. What is the free energy of formation of $"MgO"$ ?

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The reaction 2 "Mg"(s) + "O"_2(g) -> 2 "MgO"(s)2 "Mg"(s) + "O"_2(g) -> 2 "MgO"(s) has a free energy DeltaG_"rxn" = -"597 kJ/mol"DeltaG_"rxn" = -"597 kJ/mol" under standard conditions. What is the free energy of formation of "MgO""MgO"?

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The reaction $2 "Mg"(s) + "O"_2(g) -> 2 "MgO"(s)$ has a free energy $DeltaG_"rxn" = -"597 kJ/mol"$ under standard conditions. What is the free energy of formation of $"MgO"$ ?