Base your answer on the following redox reaction, which occurs spontaneously in an electrochemical cell. Zn + Cr3+ --> Zn2+ + Cr

Write the half-reaction for the reduction that occurs.

Zn(s) --> Zn^2+(aq) + 2e^- (Oxidation half reaction)

Cr^3+(aq) + 3e^- --> Cr(s) (Reduction half reaction)

Well, well, well, looks like we've got ourselves a redox reaction here! Time to break out some humor to tackle this one. Ready?

Alrighty then! In the left corner, we have our friend Zn, all set to be the hero of reduction! And in the right corner, we've got the notorious Cr3+ ready to have its electrons taken away. Who will win this electrifying battle? Let's see!

Now, reduction is all about gaining electrons, so Zn wants to show off its electron-collecting skills and become the champion. So, here's our hilarious half-reaction for the reduction:

Cr3+ + 3e- → Cr

And there we have it, folks! Zn might've won this comedic round, but don't worry, Cr3+ will find its electrifying comeback. Stay tuned for more electrifying reactions, brought to you by yours truly, the Clown Bot!

To determine the half-reaction for the reduction that occurs in the given redox reaction, we need to identify the species being reduced and the change in oxidation states.

In this redox reaction, the Cr3+ ion is being reduced because it is gaining electrons. The Cr3+ ion has an oxidation state of +3 in the reactant side and an oxidation state of 0 in the product side.

Therefore, the half-reaction for the reduction that occurs is:

Cr3+ + 3e- → Cr

This half-reaction represents the reduction of Cr3+ to Cr, where 3 electrons are gained by Cr3+ to form Cr with an oxidation state of 0.

To determine the half-reaction for the reduction that occurs in the given redox reaction, we need to identify the changes in oxidation states of the elements involved.

In the reaction: Zn + Cr3+ --> Zn2+ + Cr

We know that Zn is being oxidized since it goes from an oxidation state of 0 to +2. The oxidation state of Cr remains unchanged as it goes from +3 to 0. Therefore, Zn is the reducing agent.

The half-reaction for the reduction can be written by showing how Zn is gaining electrons. Since Zn is being reduced, it gains two electrons to form Zn2+. Here is the half-reaction for the reduction:

Zn2+ + 2e- --> Zn

This half-reaction shows the reduction of Zn2+ ions to Zn metal by gaining two electrons.