Question

If under a given set of conditions the reaction ????→????A→B occurs with Δ????=−14 kJ/mol,ΔG=−14 kJ/mol, and the reaction ????→????C→B occurs with Δ????=+16 kJ/molΔG=+16 kJ/mol , then

Answer 1

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.

Step-by-step 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.