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Ya Gao
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Joined: Fri Sep 29, 2017 7:04 am
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Postby Ya Gao » Sun Feb 18, 2018 10:51 pm

Hey guys, I'm having trouble solving question 14.37a.
Determine the potential of the following cell: Pt(s)|H2 (g. 1.0 bar) | HCl (0.075M)||HCl(1.0 mol\L) |H2(1.0 bar)|Pt(s)
Can someone please tell me how to put in the data. Thanks!

Adrienne Dang 1B
Posts: 30
Joined: Fri Sep 29, 2017 7:05 am

Re: 14.37

Postby Adrienne Dang 1B » Sun Feb 18, 2018 11:16 pm

First you need to write both of the half reactions, the reduction reaction and the oxidation reaction. Each half reaction in this case has a standard potential of 0. So when you plug that into the equation for the standard potential of the cell (subtracting that of the anode from the cathode potential), you get 0.00V. You can then plug that into the nernst equation, plug in the values given for Q (the pressures and the concentrations), and then solve for E.

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