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Question

If K1 and K2 are the equilibrium constants at temperature T1 and T2, where T2>T1, then :

A
K2=K when ΔH is 0
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B
K2>K1 when ΔH is +ve
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C
K2<K1 when ΔH is -ve
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D
K2<K1 when ΔH is +ve
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Solution

The correct options are
A K2=K when ΔH is 0
B K2>K1 when ΔH is +ve
C K2<K1 when ΔH is -ve
The van't Hoff equation is logK2K1=+ΔH2.303R[1T11T2]=>ΔH2.303R[T2T1T1T2].
Here, K1 and K2 are the values of the equilibrium constants at temperatures T1 and T2 respectively.
ΔH is the enthalpy of the reaction and R is the ideal gas constant.
When ΔH=0 and T2>T1, then term ΔH2.303R[1T11T2] is zero.
Hence, K2K1=1 or K2=K1
When ΔH>0 and T2>T1, then the term ΔH2.303R[1T11T2]>0 .
Hence, K2K1>1 or K2>K1
When ΔH<0 and T2>T1, then the term ΔH2.303R[1T11T2]<0.
Hence, K2K1<1 or K2<K1

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