University College - Chemistry Chem 112A Lecture 27: Standard Zinc Hydrogen Cell

• School: WUSTL
• Department: University College - Chemistry
• Course: University College - Chemistry Chem 112A
• Professor: D' Arcy

Document Summary

G anode = g f (zn2+) + 2 g f e- - g r (zn) G cathode = g f (h2o) + 1/2 g f(h2) - g f(h3o+) - g f (e-) = -237. 18 + (0) [-237. 18 - g f (e-)] G f for the standard h electrode = 0 (by convention) + 2(h3o+ + 1e h2o + h2) Zn + 2h3o+ + 2e- -> zn2+ + 2e- + 2h2o + h2. G cell = g f (anode) + 2 g f (cathode) = g f (anode) = -147. 06 kj/mol. E - half cell potential = -ne, anode*f*e anode + 2(-ne, cathode)*f*e cathode. She is a reference for voltage of any other electrode. G cell = -2*f*e anode + 0 = -2f( e ) = -2f(e anode + e cathode) E cell = e cathode, red - e anode, red = 0. 34 (-0. 76) = 1. 10 v. The higher the reduction potential, the more easily something is reduced.