Consider this combination reaction:

2Mg (s) + O2 (g) →2MgO (s) ΔH=-1204 kJ

What is the enthalpy for the decomposition of 1 mole of MgO (s) into Mg (s) and O2 (g) ?

Question

Chemistry

Adrien Frank

21 August, 18:04

Consider this combination reaction:

2Mg (s) + O2 (g) →2MgO (s) ΔH=-1204 kJ

What is the enthalpy for the decomposition of 1 mole of MgO (s) into Mg (s) and O2 (g) ?

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Answers (1)

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Johnathan Reynolds · Answer 1

Since the decomposition of MgO is the reverse of the reaction you have given us. The sign will be reversed:

2MgO - > 2Mg + O2 = 1204 kJ

Divide by two:

MgO - > Mg + 1/2 O2 =

602 kJ

Consider this combination reaction:2Mg (s) + O2 (g) →2MgO (s) ΔH=-1204 kJWhat is the enthalpy for the decomposition of 1 mole of MgO (s) into Mg (s) and O2 (g) ?

Consider this combination reaction:

2Mg (s) + O2 (g) →2MgO (s) ΔH=-1204 kJ

What is the enthalpy for the decomposition of 1 mole of MgO (s) into Mg (s) and O2 (g) ?