Question

consider the reaction cl₂(g) + br₂(g) → 2 brcl(g) at 25 °c. the change in the free energy under standard conditions is 25.9 kj/mol. is this reaction spontaneous as written under standard conditions? a yes, because δg° > 0. b no, because δg° > 0.

Explanation:

Step1: Recall spontaneity rule

For a reaction, the sign of standard Gibbs free energy change ($\Delta G^\circ$) determines spontaneity. If $\Delta G^\circ < 0$, the reaction is spontaneous; if $\Delta G^\circ > 0$, it is non - spontaneous.

Step2: Analyze given $\Delta G^\circ$

The given $\Delta G^\circ$ for the reaction $\ce{Cl2(g) + Br2(g) -> 2BrCl(g)}$ is $25.9\space kJ/mol$, which means $\Delta G^\circ>0$.

Answer:

B. No, because $\Delta G^\circ > 0$.