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A reaction has DeltaH=-33KJ and DeltaS=-...

A reaction has `DeltaH=-33KJ` and `DeltaS=-58(J)/(H)` . This reaction would be:

A

spontanceous at all temperatures

B

non-spontaneous at all temperatures

C

spontaneous above a certain temperature

D

spontaneous below a certain temperature

Text Solution

Verified by Experts

The correct Answer is:
B
`DeltaG=underset(-ve)undersetdarr((DeltaH))-Tunderset(-ve)undersetdarr((DeltaS))`
Since both are `-ve` , the reaction would have a `-veDeltaG` below a temperature of `(33000)/(58)K(=569K)` .
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