Homework Help: Chemistry

Posted by Diana on Monday, November 15, 2010 at 12:28pm.

Consider an electrochemical cell based on the following cell diagram:

Pt | Pu3+(aq), Pu4+(aq) || Cl2(g), Cl−(aq) | Pt

Given that the standard cell emf is 0.35 V and that the standard reduction potential of chlorine is 1.36 V, what is the standard reduction potential E°(Pu4+/Pu3+), in volts? [Enter only a number.]

Chemistry - DrBob222, Monday, November 15, 2010 at 5:37pm
Pu+3 ==> Pu+4 + e Eo = ??
Cl2 + 2e ==> 2Cl^- Eo 1.36
============================
2Pu+3 + Cl2 ==> 2Pu+4 + 2Cl^- Ece.. = 0.35
What is ?? + 1.36 = 0.35
Solve for ?? which will be the oxidation potential (because that's the way the half cell is written above) so change the sign for the reduction problem (what the problem is asking).
Chemistry - Josh, Tuesday, May 1, 2012 at 11:29pm
Cl is gaining elections which means it is the reduction half reaction. Reduction is associated with the Cathode.

E(cell) = E(cathode) - E(anode)

0.35v = 1.36v - E(anode)
solving for E(anode) gives you 1.01v

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