## 6N.1

$E_{cell} = E_{cell}^{\circ}-\frac{RT}{nF}\ln Q$

KNguyen_1I
Posts: 101
Joined: Sat Aug 17, 2019 12:16 am

### 6N.1

6N.1 Calculate the equilibrium constants for the following
reactions:
(b) In3+(aq) + U3+(aq) = In2+(aq) + U4+(aq)

I don't know how to do this problem because I can't find the reduction potentials for In 3 to 2+ and the same for Uranium?

Hiba Alnajjar_2C
Posts: 108
Joined: Fri Aug 09, 2019 12:17 am

### Re: 6N.1

Did you check Appendix 2B? The standard reduction potentials can be found there. :)

Kristina Rizo 2K
Posts: 105
Joined: Wed Sep 18, 2019 12:19 am

### Re: 6N.1

The reaction potentials are found on pg A16-17 for the seventh edition book.

Long Luong 2H
Posts: 51
Joined: Thu Sep 19, 2019 12:16 am

### Re: 6N.1

From Appendix 2B,
In3+ + e- -> In2+ is -0.49V
U4+ + e- -> U3+ is -0.61V

Morgan Carrington 2H
Posts: 54
Joined: Wed Nov 14, 2018 12:22 am

### Re: 6N.1

KNguyen_1I wrote:6N.1 Calculate the equilibrium constants for the following
reactions:
(b) In3+(aq) + U3+(aq) = In2+(aq) + U4+(aq)

I don't know how to do this problem because I can't find the reduction potentials for In 3 to 2+ and the same for Uranium?

For part a of this problem, how do you calculate the cell potential of the cell? i keep getting -0.45 V, but that produces the wrong K value.

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