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Question

If the bond dissociation energy of XY, X2, Y2 (all are gaseous diatomic molecules) are in the ratio of 1:1:0.5 and enthalpy for the formation of XY is -200kJ/mol. The bond dissociation energy of X2 will be:

A
200 KJ/ mol
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B
100 KJ/ mol
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C
800 KJ/ mol
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D
300 KJ/ mol
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Solution

The correct option is B 800 KJ/ mol
Solution:- (C) 800kJ/mol
Given that the bond dissociation energy of XY,X2 and Y2 are in the ratio 1:1:0.5.
Let the bond energy of XY,X2 and Y2 be 2x,2x and x respectively.
12X2+12Y2XY;ΔH=200kJ/mol
For the above reaction,
ΔH=B.E.(reactant)B.E.(product)
200=(12×2x+12×x)(2x)
200=32x2x
x=(200)×(2)=400
Therefore,
Bond dissociation energy of X2=2×400=800kJ/mol
Hence the bond dissociation energy of X2 is 800kJ/mol.

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