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. Cu2+(aq)/ Cu(s) // Ag(s) / Ag+(aq)
B. 2Ag+(aq)/ Cu2+(aq)// 2Ag(s)/ Cu(s)
C. Ag+(aq) / Cu2+(aq)// Cu(s) / Ag(s)
D. Cu(s) / Cu2+(aq)// Ag+(aq) / Ag(s)
E. Cu(s) / Cu2+(aq) // 2Ag+(aq) / 2Ag(s)
What reaction is occurring at the anode?
A. Cu2+ + 2e– --> Cu
B. Cu ---> Cu2+ + 2e–
C. Ag+ + e–---> Ag
D. Ag ---> Ag+ + e–
And what do you think? Don't just guess. Tell me why you think that.
To determine the correct cell notation at standard state conditions, we need to understand the components of a cell notation. The general form of a cell notation is:
Anode (oxidation) | Electrolyte || Electrolyte | Cathode (reduction)
In this case, we have the following half-reactions for the given balanced equation:
1. Oxidation half-reaction (anode): 2 Ag+ (aq) --> 2 Ag(s) + 2e–
2. Reduction half-reaction (cathode): Cu(s) --> Cu2+ (aq) + 2e–
The correct cell notation should have the anode on the left side and the cathode on the right side, separated by double vertical lines. The correct electrolytes must also be included.
Let's analyze the options:
A. Cu2+(aq)/ Cu(s) // Ag(s) / Ag+(aq)
This option does not match the given balanced equation sequence. The anode and cathode are reversed.
B. 2Ag+(aq)/ Cu2+(aq)// 2Ag(s)/ Cu(s)
This option correctly matches the given balanced equation sequence. The anode (oxidation) includes 2Ag+ (aq) and Cu(s), while the cathode (reduction) includes 2Ag(s) and Cu2+ (aq).
C. Ag+(aq) / Cu2+(aq)// Cu(s) / Ag(s)
This option does not match the given balanced equation sequence. The anode and cathode are reversed.
D. Cu(s) / Cu2+(aq)// Ag+(aq) / Ag(s)
This option does not match the given balanced equation sequence. The anode and cathode are reversed.
E. Cu(s) / Cu2+(aq) // 2Ag+(aq) / 2Ag(s)
This option does not match the given balanced equation sequence. The anode and cathode are reversed.
Based on the analysis, the correct cell notation for the given balanced equation at standard state conditions is:
B. 2Ag+(aq)/ Cu2+(aq)// 2Ag(s)/ Cu(s)
To determine the reaction occurring at the anode, we need to identify the half-reaction at the anode, which represents oxidation.
The correct half-reaction for oxidation (anode) in the given balanced equation is:
A. Cu2+ + 2e– --> Cu
So the reaction occurring at the anode is:
A. Cu2+ + 2e– --> Cu