For the reaction at `298 K` `2A+B rarr C` `DeltaH=400 kJ mol^(-1)` and `DeltaS=0.2 kJ K^(-1) mol^(-1)` At what temperature will the reaction becomes spontaneous considering `DeltaH` and `DeltaS` to be contant over the temperature range.

For the reaction at `298 K` `2A+B rarr C` `DeltaH=400 kJ mol^(-1)` and

1.	For the reaction at `298 K` `2A+B rarr C` `DeltaH=400 kJ mol^(-1)` and `DeltaS=0.2 kJ K^(-1) mol^(-1)` At what temperature will the reaction becomes spontaneous considering `DeltaH` and `DeltaS` to be contant over the temperature range.
Answer» Correct Answer - 2000K From the expression, `DeltaG=DeltaH-TDeltaS` Assumingb the reaction at equilibrium , `DeltaT` for the reaction would be : `T=(DeltaH-DeltaG)(1)/(DeltaS)` `(DeltaH)/(DeltaS)(DeltaG=0` at equilibrium ) `=(400 kJ "mol"^(-1))/(0.2 kJ^(-1)"mol"^(-1))` T=2000 K For the reaction to be spontaneous, `DeltaG` must be negative . Hence , for the given reaction to be spontaneous, T should be greater than 2000 K.

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For the reaction at `298 K` `2A+B rarr C` `DeltaH=400 kJ mol^(-1)` and `DeltaS=0.2 kJ K^(-1) mol^(-1)` At what temperature will the reaction becomes spontaneous considering `DeltaH` and `DeltaS` to be contant over the temperature range.

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