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Question

For a given reaction, ΔH=35.5kJmol−1 and ΔS=83.6kJmol−1. The reaction is spontaneous at: (Assume that ΔH and ΔS do not vary with temperature)

A
T > 425 K
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B
all temperatures
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C
T > 298 K
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D
T < 425 K
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Solution

The correct option is A T > 425 KSolution:- (A) T>425KThe reaction is {spontaneousif ΔG<0non-spontaneousif ΔG>0As we know that,ΔG=ΔH−TΔS∵ The reaction is spontaneous.∴ΔG<0ΔH−TΔS<0⇒T>ΔHΔSGiven:-ΔH=35.5KJ/mol=35500J/molΔS=83.6J/mol−K∴T>3550083.6⇒T>425KHence the reaction will be spontaneous at T>425K.

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