For the following balanced equation: 2 Ag+ (aq) + Cu(s) <<->> Cu2+ (aq) + 2 Ag(s)
Which letter corresponds to the correct cell notation at standard state conditions?
A. 2Ag+(aq) | Cu2+(aq) || 2Ag(s) | Cu(s)
B. Cu(s)| Cu2+(aq) || Ag+(aq) | Ag(s)
C. Ag+(aq) | Cu2+(aq) || Cu(s) | Ag(s)
D. Cu2+(aq)| Cu(s) || Ag(s) | Ag+(aq)
E. Cu(s) | Cu2+(aq)|| 2Ag+(aq) | 2Ag(s)
What reaction is occurring at the anode?
A. Cu -> Cu2+ + 2e–
B. Cu2+ + 2e– -> Cu
C. Ag+ + e– -> Ag
D. Ag -> Ag+ + e–
Is it B , A?
yes.
To determine the correct cell notation for the given balanced equation, we need to understand the structure of cell notation. The general format for cell notation is:
Anode (oxidation) | Electrolyte Solution || Electrolyte Solution | Cathode (reduction)
Based on the balanced equation:
2 Ag+ (aq) + Cu(s) <<->> Cu2+ (aq) + 2 Ag(s)
We can identify the oxidation half-reaction and the reduction half-reaction. The oxidation half-reaction occurs at the anode, where Cu is being oxidized to Cu2+:
Cu -> Cu2+ + 2e–
The reduction half-reaction occurs at the cathode, where Ag+ is being reduced to Ag:
Ag+ + e– -> Ag
Now, let's analyze the given options:
A. 2Ag+(aq) | Cu2+(aq) || 2Ag(s) | Cu(s)
B. Cu(s) | Cu2+(aq) || Ag+(aq) | Ag(s)
C. Ag+(aq) | Cu2+(aq) || Cu(s) | Ag(s)
D. Cu2+(aq) | Cu(s) || Ag(s) | Ag+(aq)
E. Cu(s) | Cu2+(aq) || 2Ag+(aq) | 2Ag(s)
The correct cell notation at standard state conditions is option C:
Ag+(aq) | Cu2+(aq) || Cu(s) | Ag(s)
Now let's determine the reaction occurring at the anode. We already identified that the oxidation half-reaction occurs at the anode. From the given balanced equation, the oxidation half-reaction is:
Cu -> Cu2+ + 2e–
Therefore, the correct answer is option A:
Cu -> Cu2+ + 2e–
So, the correct answers are:
1. C
2. A