Answer
The reaction will be favorable if Gibb's Free Energy is negative. Recall the equation for Gibb's Free Energy: $\Delta G^{\circ}=\Delta H^{\circ}-T\Delta S^{\circ}$. From this, we see that when looking for a favorable reaction, it is best for energy to be negative and for entropy to be positive. (Entropy is positive when there are more moles of gaseous products, and it will be negative when there are more moles of gaseous reactants.) Seeing this, we see that energy favors the reaction and entropy does not favor the reaction.
Work Step by Step
The reaction will be favorable if Gibb's Free Energy is negative. Recall the equation for Gibb's Free Energy: $\Delta G^{\circ}=\Delta H^{\circ}-T\Delta S^{\circ}$. From this, we see that when looking for a favorable reaction, it is best for energy to be negative and for entropy to be positive. (Entropy is positive when there are more moles of gaseous products, and it will be negative when there are more moles of gaseous reactants.) Seeing this, we see that energy favors the reaction and entropy does not favor the reaction.
