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Question

If for a particular reversible reaction at:
KC=57 at 355C and KC=69 at 450C then:

A
ΔH<0
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B
ΔH>0
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C
ΔH=0
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D
ΔH whose sign can't be determined
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Solution

The correct option is B ΔH>0
With increase in temperature, KC increases, this means the forward reaction increases with increase in temperature. Hence, forward reaction is endothermic.

Using equation
logK2K1=ΔH2.303R(1T11T2)log6957=ΔH2.303R(16281723)
From here, you will get
ΔH=+ve

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