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 .

Explanation

Data given ,
`2A+B to C` at 298 K
`DeltaH="400 KJ mol"^(-1)`
`DeltaS=0.2 J K^(-1) "mol"^(-1)`
T=298 K `[DeltaG=DeltaH-TDetlaS]`
If `DeltaG=0`
`DeltaH-TDeltaS=0`
`DeltaS=(DeltaH)/T`
For `DeltaG=0, DeltaS=(DeltaH)/T=400/0.2 =4000/2`=2000 K
`therefore` T=2000 K
At 2000 K , the reaction is in equilibrium . So , above 2000 K, the reaction will be spontaneous .