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For the reaction, 2A+B to C,DeltaH=400kJ...

For the reaction, `2A+B to C,DeltaH=400kJ*mol^(-1)` & `DeltaS=0.2kJ*K^(-1)*mol^(-1)` at 298K. At what temperature will the reaction become spontaneous considering `DeltaH,DeltaS ` to be constant over the temperature range?

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We know, `DeltaG=DeltaH-TDeltaS`. For a spontaneous reaction at a given temperature and pressure `Delta G lt 0`.
Given: `DeltaH=400kJ*mol^(-1)` and
`DeltaS=0.2kJ*K^(-1)*mol^(-1)`
`DeltaS=0.2kJ*K^(-1)*mol^(-1)`
So, `DeltaG=(400-Txx0.2)kJ*mol^(-1)`
According to this relation, `DeltaG` will be `lt0` when `T xx0.2gt400` i.e., `Tgt2000K`.
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