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Question

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

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

## The correct option is A T>425K The reaction is{spontaneous ifΔG<0non-spontaneous if ΔG>0 As we know that, ΔG=ΔH−TΔS ∵ The reaction is spontaneous. ∴ΔG<0 ΔH−TΔS<0 ⇒T>ΔHΔS Given:- ΔH=35.5 KJ/mol=35500J/mol ΔS=83.6 J/mol.K ∴T>3550083.6 ⇒T>425 K Hence the reaction will be spontaneous at T>425K

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