Achieve #17

[Katie L 2I]

Can I get a walkthrough of Achieve #17 on the electrochemistry homework, on how to find the potential of the standard hydrogen electrode?

[Alyssa Bercero 3H]

You use the Nernst equation, solving for E. E° is 0 under standard conditions and then you need moles of electrons and Q. There are 2 moles because H+ + 2e- —> H2. Q can be found by P/R, which would be Pressure of H2/[H+].

[Katie L 2I]

thank you for your help!

To expand on this, I also found another way to do this with a different version of the Nernst equation, using log instead of natural logs.

I used Eº - (0.0592/n) * log(Q), then plugged in the corresponding values.

How are the two equations linked?

[Maddy Barron 1L]

These equations are linked because that is the 0.0592(?) is the constant you would get by simplifying the numerator of the Nernst equation! He went over it in class, its lets of a hassle to do it that way with it already simplified. Then you just plug in your values and go from there.