The bond dissociation enthalpy of X2 bond H calculated from the given data is_____ kJ mol–1. (Nearest integer) M+X–(s) M+(g) + X– (g) lattice H = 800 kJ mol–1 M(s) M(g) sub H = 100 kJ mol–1 M(g) M+(g)

Question

The bond dissociation enthalpy of X2 bond H calculated from the given data is_____ kJ mol–1. (Nearest integer) M+X–(s) M+(g) + X– (g) lattice H = 800 kJ mol–1 M(s) M(g) sub H = 100 kJ mol–1 M(g) M+(g) + e– (g) i H = 500 kJ mol–1 X(g) + e– (g) X–(g) eg H = –300 kJ mol–1 M(s) + 1 X2 (g) M+X–(s) f H = –400 kJ mol–1 [Given : M+X– is a pure ionic compound and X forms a diatomic molecule X2 in gaseous state]

Prashant Kotian · Accepted Answer

Correct answer: .. M(s) + 1 X2 (g)    f H Hsub. M(s) HLattice M+(g) + X–(g) M+X– HLattice ½HBDE Henergy X(g) According to Hess's law Hf = Hsub. + HI.E1 + 2 1 HBDE + Heg + HLattice – 400 = 100 + 500 + 1 HBDE + (–300) – 800 + 100 = 1 HBDE ; HBDE = 200 kJ/mol

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