For the reaction at 298 K : 2A +B to C DeltaH="400 KJ mol"^(-1) , DeltaS ="0.2 JK"^(-1) "mol"^(-1) Determine the temperature at which the reaction would be spontaneous .

For the reaction at 298 K : 2A +B to C DeltaH="400 KJ mol"^(-1) , Del

1.	For the reaction at 298 K : 2A +B to C DeltaH="400 KJ mol"^(-1) , DeltaS ="0.2 JK"^(-1) "mol"^(-1) Determine the temperature at which the reaction would be spontaneous .
Answer» Solution :Given: T=298 K `DeltaH=400 "J mol"^(-1) =400 "J mol"^(-1)` `DeltaS=0.2 JK^(-1) mol^(-1)` `DELTAG=DeltaH-TDeltaS` If T=2000 K `DeltaG`=400 -(0.2 x 2000) =0 if T > 2000 K `DeltaG` will be negative The reaction WOULD be spontaneus only BEYOND 2000 K .