If under a given set of conditions the reaction →→b occurs with δ=−14 kj/mol,δg=−14 kj/mol, and the reaction →→b occurs with δ=+16 kj/molδg=+16 kj/mol , then

Reaction A to B is feasible and exothermic, C to B is not feasible and would be endothermic, given this, the reaction that is feasible is B to C, because the opposite direction of the reaction changes the sign of ΔG and ΔH.

Explanation:

When ΔG < 0 in any chemical reaction, it means that the reaction is feasible, but if ΔG > 0, the reaction cannot occur.

When ΔH < 0, it means that the reaction is exothermic, it means that the reaction releases energy, but if ΔH > 0, it meas that the reaction is endothermic, so it needs energy to be feasible.

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