Red-Half - Ag+(aq) + 1e --> Ag(s)
Ox-Half - Cu(s) --> Cu+2(aq) + 2e
Overall Rxn: 2Ag+(aq) + Cu(s) --> 2Ag(s) + Cu2+(aq)
This is in relation to voltaic cells though. Ag being the cathode, and Cu being the anode.
Lol, no, I was talking about oxidation and reduction reactions, especially those relating to electrochemistry.
I guessed redox because an element gains an electron, thus the electron loses energy. Oxidation on the other hand would require an input of energy to remove an electron. So I guessed...
Homework Statement
Sn + 2 Ag+ --> Sn2+ + 2 Ag
a) Calculate the standard voltage of a cell involving the system above. (I got +0.94 Volts).
b) What is the equilibrium constant for the system above? (I got 5.71 E 31)
c) Calculate the voltage at 25 degrees celsius of a cell involving the system...
Seems like a strange question, but it just appeared on one of my tests. My guess would be redox, but what is the logic behind the answer?
Thanks for the help!