By using ΔGf° values as 2Mg(s) + O₂(g) → 2MgO(s) the value of ΔG° is -1139.2 kJ/mol.
Calculate ΔG° for the following reaction:
The response is as follows:
2Mg(s)+ O2(g) -------> 2MgO (s)
Thus,
ΔG° = (2ΔGf°( MgO(s))- [2ΔGf°(Mg(s))+ΔGf°(O2(g))]
To solve for the reaction's ΔG°, take the thermodynamic data from Appendix 2 and
replace them with -569.6 kJ/mol for the ΔG° of MgO(s),
0 kJ/mol for the ΔG° of Mg(s), and
0 kJ/mol for the ΔG° of O2(g).
ΔG° = 2(-569.6) - [2*0 + 0]
ΔG°= -1139.2 kJ/mol.
As a result, the reaction's ΔG° is -1139.2 kJ/mol.
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