CHEM 112 Lecture Notes - Lecture 3: Nernst Equation, Reaction Quotient, Electrochemistry
Document Summary
Zfecell = -zfeo cell + rt ln q. Ecell = eo cell rt/zf ln q. This equation shows that the value of the reaction quotient affects whether the forward or reverse reaction is favoured under a particular set of conditions. If t = 298. 15 k, standard temperature, and we change from ln q to log q (factor of 2. 303), then the. When q > 1, ecell < e o cell. When q < 1 ecell > e o cell. E o cell = e o (ag+ /ag) - e o (fe3+/fe2+) = 0. 800 0. 771 v = 0. 029 v. [fe2+] = 0. 10 m [fe3+] = 0. 20 m [ag+ ] = 1. 00 m 0. 0592 v [fe3+] Pt|h2 (1 bar)|h+ (x m)||h+ (1. 0 m)|h2 (1 bar)|pt(s) 2 h+ (1 m) + 2 e - h2 (g, 1 bar) H2 (g, 1 bar) 2 h+ (x m) + 2 e . 2 h+ (1 m) 2 h+ (x m)
