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For a given reaction, Delta H = 35.5 kJ ...

For a given reaction, `Delta H = 35.5 kJ mol^(-1)` and `Delta S = 83.6 JK^(-1) mol(-1)`. The reaction is spontaneous at : (Assume that `Delta H and Delta S` do not vary with temperature)

A

`T gt 298 K`

B

`T lt 425 K`

C

`T gt 425 K`

D

All temperatures

Text Solution

Verified by Experts

The correct Answer is:
C
`DeltaG= DeltaH- TDeltaS`
For spontaneous reaction, `DeltaG` must be negative . For negative value of `DeltaG, DeltaH` should be lesser than `TDeltaS`. It is possible when `T gt 425K`
`DeltaH= 35.5 KJ//mol= 35500 J//mol`
`TDeltaS= (425) (83.6) = 35530`
`T DeltaS gt Delta H`
Hence, the reaction is spontaneous.
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