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"#?

Answer 1

-298.5 kJ/mol

-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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Answer 2

Peyton Adams

The free energy of formation of MgO is -597 kJ/mol.

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Answer from HIX Tutor

When evaluating a one-sided limit, you need to be careful when a quantity is approaching zero since its sign is different depending on which way it is approaching zero from. Let us look at some examples.

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

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"#?