Hey guys, I just did a lab on electrochem but we haven't started learning this in our lectures so I'm not too confident on it. One of the lab question asks us to calculate the expected cell voltage. From reading the text book, this is what I did: The reaction was 2Ag+ + Cu -> 2Ag + Cu2+ I added reduction potentials of Ag and Cu to get 0.46V for the standard voltage. Then I used the nersnt eq'n E= 0.46 -(0.05915/n)*logQ What I'm not sure about is... We used 0.1 M AgNO3 and Cu(NO3)2, so would n be 2 or 0.2? And would Q= [0.1 Cu2+]/[0.1 Ag+]^2*=10? Help would be appreciated!