please verify my answer:
Consider the following REDOX reaction:
Zn(s) + Pb+2(aq) �� Zn+2(aq) + Pb(s)
a. Write the oxidation and reduction half-cell reactions.
Zn(s) + Pb+2(aq) �� Zn+2(aq) + Pb(s)
+2 +4 +2 +4
Zn(s)->Zn2+(aq)+2e- (zinc is oxidized)
Pb2+(aq)+2e- ->Pb(s)(lead is reduced)
b. Show this reaction in shorthand notation. (2 marks)
Zn(s)| Zn2+(aq) || Pb2+(aq) | Pb(s)
If it's wrong please tell me how. Thank you for your help :)
How could u say that the on undergoes reduction as positive charge on it show that it perform oxidation as during after an atom loses electron it get + charge on it .
Your answer is almost correct, but there is a small mistake in the oxidation half-cell reaction. The correct oxidation half-cell reaction is:
Zn(s) -> Zn2+(aq) + 2e-
The charges and the number of electrons transferred should be balanced properly. Here's the corrected answer:
a. Write the oxidation and reduction half-cell reactions.
Oxidation half-reaction: Zn(s) -> Zn2+(aq) + 2e-
Reduction half-reaction: Pb2+(aq) + 2e- -> Pb(s)
b. Show this reaction in shorthand notation.
Zn(s) | Zn2+(aq) || Pb2+(aq) | Pb(s)
This notation represents a galvanic cell, where the left side represents the anode (oxidation half-reaction) and the right side represents the cathode (reduction half-reaction). The double line represents a salt bridge or a porous barrier that allows ions to flow and maintain charge balance during the reaction.
Your answers are correct! Here's a verification:
a. The oxidation half-cell reaction is:
Zn(s) -> Zn2+(aq) + 2e- (zinc is oxidized)
The reduction half-cell reaction is:
Pb2+(aq) + 2e- -> Pb(s) (lead is reduced)
b. The shorthand notation for the given reaction is:
Zn(s)|Zn2+(aq)||Pb2+(aq)|Pb(s)
Well done! Your answers are accurate.