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. Cu(s)/Cu2+(aq)//Ag+(aq)/Ag(s)
B. Cu2+(aq)/ Cu(s)// Ag(s)/ Ag+(aq)
C. Ag+(aq)/ Cu2+(aq)// Cu(s)/ Ag(s)
D. 2Ag+(aq)/ Cu2+(aq)// 2Ag(s)/ Cu(s)
E. Cu(s)/ Cu2+(aq)// 2Ag+(aq)/ 2Ag(s)

What reaction is occurring at the anode?

A. Ag+ + e– --> Ag
B. Cu2+ + 2e– --> Cu
C. Cu--> Cu2+ + 2e–
D. Ag--> Ag+ + e–

Hint:

What are the two half equations?
Ag^+(aq) + e ==> Ag(s) and
Cu(s) ==> Cu^+2(aq) + 2e.
By convention, the anode (negative charge) is shown on the left side of the || salt bridge and the cathode (+ charged) on the right side of the bridge. Technically, I don't think ANY of them represent the equation because standard state conditions would show the aq soln at 1 M. Perhaps the problem does and you just didn't type it in; however, I think the intent of the problem is for you to pick one since "none of the above" is a choice.
Fpr #2, see my comments at your original post.

To determine the correct cell notation at standard state conditions, we need to remember the general structure of a cell notation.

The cell notation consists of two half-cells, separated by a double vertical line (||). The left half-cell represents the anode (the site of oxidation) and the right half-cell represents the cathode (the site of reduction).

Let's analyze the given options:

A. Cu(s)/Cu2+(aq)//Ag+(aq)/Ag(s)
B. Cu2+(aq)/Cu(s)//Ag(s)/Ag+(aq)
C. Ag+(aq)/Cu2+(aq)//Cu(s)/Ag(s)
D. 2Ag+(aq)/Cu2+(aq)//2Ag(s)/Cu(s)
E. Cu(s)/Cu2+(aq)//2Ag+(aq)/2Ag(s)

From the balanced equation, we can determine that copper (Cu) is being oxidized and silver (Ag) is being reduced. The species in each half-cell should match with their respective coefficients in the balanced equation.

Looking at option B, we see that Cu2+(aq) is on the left side (anode) and Cu(s) is on the right side (cathode). The silver species are also correctly placed. Thus, option B represents the correct cell notation at standard state conditions: Cu2+(aq)/Cu(s)//Ag(s)/Ag+(aq).

To determine the reaction occurring at the anode, we need to identify the oxidation half-reaction. In the balanced equation, we see that copper (Cu) is being oxidized to Cu2+. Therefore, the correct answer is:

C. Cu--> Cu2+ + 2e–