For the following balanced equation:
2Ag+(aq) + Cu(s)<->Cu2+ (aq) + 2 Ag(s)
Which letter corresponds to the correct cell notation at standard state conditions?
A. Cu(s) | Cu2+(aq) || Ag+(aq) | Ag(s)
B. Ag+(aq) | Cu2+(aq) || Cu(s) | Ag(s)
C. 2Ag+(aq) | Cu2+(aq) || 2Ag(s) | Cu(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. Cu2+ + 2e– -> Cu
B. Ag+ + e– -> Ag
C. Cu -> Cu2+ + 2e–
D. Ag -> Ag+ + e–
I thought we did this before. Tell me what you think and why.
5446
To determine the correct cell notation at standard state conditions, we need to understand the notation itself. In the cell notation, the anode is always listed on the left side and the cathode on the right side, separated by two vertical lines (||) representing the salt bridge or separator.
Let's break down the given options:
Option A: Cu(s) | Cu2+(aq) || Ag+(aq) | Ag(s)
This notation shows Cu as the anode and Ag as the cathode.
Option B: Ag+(aq) | Cu2+(aq) || Cu(s) | Ag(s)
This notation shows Ag as the anode and Cu as the cathode.
Option C: 2Ag+(aq) | Cu2+(aq) || 2Ag(s) | Cu(s)
This notation is not balanced correctly. The coefficients of 2 should not be included in the cell notation.
Option D: Cu2+(aq) | Cu(s) || Ag(s) | Ag+(aq)
This notation shows Cu2+ as the anode and Ag+ as the cathode.
Option E: Cu(s) | Cu2+(aq) || 2Ag+(aq) | 2Ag(s)
This notation shows Cu as the anode and 2Ag as the cathode.
From the above options, only option B has the correct cell notation at standard state conditions. Therefore, the answer is B.
Moving on to the second question, we need to identify the reaction occurring at the anode. In an electrochemical cell, the anode undergoes oxidation, which involves the loss of electrons.
The reaction occurring at the anode is:
Cu(s) -> Cu2+ + 2e–
Therefore, the correct answer is C, "Cu -> Cu2+ + 2e–".