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 .
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 .
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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 .