Please help verify my answer. Not confident it is right:
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 :)
See your post above.
To verify your answer, let's break it down step by step:
a. Write the oxidation and reduction half-cell reactions:
The given reaction is:
Zn(s) + Pb+2(aq) �� Zn+2(aq) + Pb(s)
To identify the oxidation and reduction half-cell reactions, we need to determine which species is being oxidized (losing electrons) and which is being reduced (gaining electrons).
In this case, Zn is going from an oxidation state of 0 to +2, indicating oxidation. Pb+2 is going from an oxidation state of +2 to 0, indicating reduction.
So, the oxidation half-cell reaction is:
Zn(s) -> Zn+2(aq) + 2e-
And the reduction half-cell reaction is:
Pb+2(aq) + 2e- -> Pb(s)
Your answer seems to be correct in identifying the oxidation and reduction half-cell reactions.
b. Show this reaction in shorthand notation:
The shorthand notation for representing the given redox reaction is known as the cell notation, which follows the format:
Anode | Anode Solution || Cathode Solution | Cathode
Based on the identified half-cell reactions, the shorthand notation for the given reaction would be:
Zn(s) | Zn+2(aq) || Pb+2(aq) | Pb(s)
So, your answer for the shorthand notation is also correct.
Overall, your answer seems accurate and correctly identifies the oxidation and reduction half-cell reactions and provides the shorthand notation for the redox reaction. Well done!