# Predicting directions of redox reactions [closed]

Hello!

In this textbook example question, how come the chlorine reaction, which has the greatest reducing power will not react? If it has the greatest E of 1.36 V that means it has most reducing stength and can "pull" electrons from both the Br and I reactions. In my mind I believed it would do so, and since the I-reaction has an even lower E than the Br-reaction the extent of oxidation would be greater for I. But in the answer they say the direct opposite, that Cl does not react and Br will only oxidize I.

Why does Cl which is the strongest oxidizing agent not do anything in this case?

• You are mixing up $\ce{Cl2}$ and $\ce{Cl-}$. $\ce{Cl2}$ is more reducing than $\ce{Br2}$, but you don't have any $\ce{Cl2}$, you only have $\ce{Cl-}$ from the dissolved $\ce{NaCl}$ – Tyberius Jan 30 at 18:51
• Oxidation power decreases in range $\ce{Cl2} \gt \ce{Br2} \gt \ce{I2}$, reduction power decreases in range $\ce{I-} \gt \ce{Br-} \gt \ce{Cl-}$ – Poutnik Jan 31 at 9:41