The values of `DeltaH` and `DeltaS` for two reactions are given below:
Reaction `A : DeltaH =- 10.0 xx 10^(3)J mol^(-1)`
`DeltaS = +30 J K^(-1) mol^(-1)`
Reaction `B: DeltaH =- 11.0 xx 10^(3)J mol^(-1)`
`DeltaS =- 100J K^(-1) mol^(-1)`
Decide whether these reactions are spontaneous or not at `300K`.

Explanation

For reaction `A: DeltaG = DeltaH - T DeltaS`
`= - 10 xx 10^(3) - 300 xx 30`
`= + 19000 J mol^(-1)`
Reaction is spontaneous.
For reaction `B: DeltaG =- 11.0 xx 10^(3) - 300 (-100)`
`=- 19000 J mol^(-1)`
Reaction is not spontaneous.