Nernst Equation

Moderators: Chem_Mod, Chem_Admin

Tamera Scott 1G
Posts: 65
Joined: Fri Sep 28, 2018 12:27 am

Nernst Equation

Postby Tamera Scott 1G » Mon Feb 25, 2019 6:11 pm

In the 6th edition of the textbook, example 14.9 Using the Nernst equation to predict a cell potential sets the reaction quotient as Zn over Cu. Why is that?

Mindy Kim 4C
Posts: 65
Joined: Fri Sep 28, 2018 12:25 am

Re: Nernst Equation

Postby Mindy Kim 4C » Tue Feb 26, 2019 12:00 pm

If you look at the reaction: Cu2+ (aq) + Zn(s) --> Zn2+(aq) + Cu(s), you have two aqueous ions and two solid metals. Remember that when setting up the reaction quotient and equilibrium constant, solids and liquids are not included. Therefore, the reaction quotient would simply be the concentrations of Zn2+ divided by Cu2+.

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: Anna Yang 1A and 1 guest