6th edition, 14.37


Moderators: Chem_Mod, Chem_Admin

Hai-Lin Yeh 1J
Posts: 89
Joined: Fri Sep 28, 2018 12:16 am
Been upvoted: 1 time

6th edition, 14.37

Postby Hai-Lin Yeh 1J » Thu Mar 07, 2019 3:15 pm

Determine the potential of each of the following cells:
(a) Pt(s) | H2(g, 1.0 bar) | HCl(aq, 0.075 m) || HCl(aq, 1.0 mol.L.-1) | H2(g, 1.0 bar) | Pt(s)

In the solutions manual, they got 2H+ + 2e- -> H2 (g) as the equation for the cathode and H2 (g) -> 2H+ (aq) + 2e- as the anode. How did that happen when there is an HCl on both sides? Where did the Cl go?

Chem_Mod
Posts: 19198
Joined: Thu Aug 04, 2011 1:53 pm
Has upvoted: 837 times

Re: 6th edition, 14.37

Postby Chem_Mod » Thu Mar 07, 2019 4:40 pm

It is a concentration cell and the Cl- is free to move around between anode and cathode.


Return to “Appications of the Nernst Equation (e.g., Concentration Cells, Non-Standard Cell Potentials, Calculating Equilibrium Constants and pH)”

Who is online

Users browsing this forum: No registered users and 1 guest