Question

# For a reaction A⇌P, the plots of [A] and [P] with time temperatrues T1 and T2 are given below. If T2>T1, the correct statement(s) is (are) (Assume ΔHθ and ΔSθ are independent of temperature and ratio of ln K at T1 to lnK at T2 is greater than T2T1. Here H, S, G and K are enthalpy, entropy, Gibbs energy and equilibrium constant, respectively.)

A
ΔHθ<0,ΔSθ<0
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B
ΔGθ<0,ΔHθ>0
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C
ΔGθ<0,ΔSθ<0
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D
ΔGθ<0,ΔSθ>0
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Solution

## The correct option is C ΔGθ<0,ΔSθ<0A⇌P (P)eq>5,(A)eq<5 Keq=[P][A]>1 ΔG0=−RT ln Keq,ΔG0<0 ln KT1ln KT2>T2T1>1 ⇒KT1KT2>1 ⇒KT2<KT1 (exothermic) ΔH0<0, since (P) at T2 < at T1 ΔG0=ΔH0−TΔS0 TΔS0=ΔH0−ΔG0 ΔS0=ΔH0−ΔG0T;(ΔH0)>(ΔG0) ΔS0<0 Also, −T1 ln KT1<−T2 ln KT2 ΔG0T1<ΔG0T2 ΔH0T1−TΔS0T1<ΔH0T2−TΔS0T2 It is possible only if ΔS0<0.

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