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

To determine whether the reactions A and B are spontaneous at 300 K, we need to calculate the Gibbs free energy change (ΔG) for each reaction using the formula:

\[ \Delta G = \Delta H - T \Delta S \]

where:
- ΔG is the change in Gibbs free energy,
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