Question

Find ΔG° for the reactions in Problem 20.51 using ΔHf° and S° values.

Answer 1

The value of ΔG° (gibbs free energy change)of the given reaction is -1131.94kj .

Given ,

Balanced chemical equation is given by,

2Mg(s) + O2 (g) → 2MgO (s)

Here , the standard enthalpy of Mg  and O2 gas are zero because they are in the most stable state .

thus , the value of ΔG°rxn is given by ,

ΔG°rxn = ΔG°(products ) - ΔG°(reactants )

ΔG°rxn = [2×(-565.97 )] - 0

ΔG°rxn = 2×(-565.97)

ΔG°rxn = -1131.94kj

Hence , the value of ΔG° of the given reaction is -1131.94kj .

What is a balance chemical reaction ?

A balanced chemical reaction is a type of reaction which include the reactants and products in same amount i.e. the no of mole on both side of the reaction is remains same or balanced .

Learn more about chemical reaction here :

brainly.com/question/1893305

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Question :

Calculate ΔG° for the reaction using ΔG°f values :

2Mg(s) + O2 (g) → 2MgO (s)

Find the ΔG° for the reaction using ΔH°f and S° values .