From the following values of `DeltaH and DeltaS`, decide whether or not these reaction are feasible at 298 K.
Reaction A : `DeltaH =- 10.5 xx 10^3 J mol^(-1), DeltaS = + 31J K^(-1) mol^(-1)`
Reaction B : `DeltaH = - 11.7 xx 10^3 J mol^(-1), DeltaS = - 105 J K^(-1) mol^(-1)`

Explanation

To determine whether the reactions are feasible at 298 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 Gibbs free energy change,
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