Enthalpy of bond dissociation, combustion and formationMedium
Bond Dissociation Enthalpy Calculation
The bond dissociation enthalpy of X2 
calculated from the given data is _______ kJ mol–1. (Nearest integer)
M+X–(s) → M+(g) + X–(g) ΔH°lattice = 800 kJ mol–1
M(s) → M(g) ΔH°sub = 100 kJ mol–1
M(g) → M+(g)– + e–(g) ΔH°i = 500 kJ mol–1
X(g) + e–(g) → X–(g) ΔH°eg = –300 kJ mol–1
M(s) +
X2(g) → M+X–(s) ΔH°f = –400 kJ mol–1
[Given : M+X– is a pure ionic compound and X forms a diatomic molecule X2 is gaseous state]
calculated from the given data is _______ kJ mol–1. (Nearest integer) M+X–(s) → M+(g) + X–(g) ΔH°lattice = 800 kJ mol–1
M(s) → M(g) ΔH°sub = 100 kJ mol–1
M(g) → M+(g)– + e–(g) ΔH°i = 500 kJ mol–1
X(g) + e–(g) → X–(g) ΔH°eg = –300 kJ mol–1
M(s) +
X2(g) → M+X–(s) ΔH°f = –400 kJ mol–1[Given : M+X– is a pure ionic compound and X forms a diatomic molecule X2 is gaseous state]
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