3 posts • Page 1 of 1
I believe you are supposed to determine this based on their reduction potentials. If you look at the table of reduction potentials, the reduction of tin has a lower potential than hydrogen, which means that tin is less likely to be reduced than hydrogen. Based on this information, you can infer that if hydrogen and tin were put into a reaction together, then hydrogen would be reduced (cathode) while tin would be oxidized (anode). Hope this helps!
You can also tell which one is the cathode and anode by calculating the E(not)cell through trial and error; the values you use to end up with an E(not)cell that is positive will tell you which species is reduced and which is oxidized.
Who is online
Users browsing this forum: No registered users and 7 guests