For a given reaction, DeltaH=35.5 KJ "mo...

For a given reaction, `DeltaH=35.5 KJ "mol"^(-1)` and `DeltaS=83.6 JK^(-1) "mol"^(-1)`. The reaction is spontaneous at: (Assume that `DeltaH and DeltaS` so not vary with temperature)

`T gt 425 K`

All temperatures

`T gt 298 K`

`T lt 424 K`

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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)

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