Problem: 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)?

FREE Expert Solution

To get the enthalpy of decomposition, reverse the equation and ΔH then divide the ΔH by 2:

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

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

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Problem Details

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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