AP Chemistry : Cell Potential Under Non-standard Conditions
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Example Questions
Example Question #1 : Cell Potential Under Non Standard Conditions
Consider an electrochemical cell that has the following overall reaction:
2 H+(aq) + Sn (s) -> Sn2+ (aq) + H2 (aq)
Which of the following changes would alter the measured cell potential?
Adding SnCl2 to the cathode.
All of the above.
Lowering the pH in the cathode.
Increase the pH in the cathode.
Increasing the H2 pressure in the cathode.
All of the above.
All of these changes would change Q and thus change the measured cell potential.
Example Question #2 : Cell Potential Under Non Standard Conditions
For the following cell reaction:
2 Al (s) + 3 Mn2+ (aq) -> 2 Al3+ (aq) + 3 Mn (s)
predict if the cell potential Ecell will be larger, or smaller than Eocell for the following conditions:
[Al3+] = 2.0 M; [Mn2+] = 1.0 M.
Smaller
Can not be determined
Identical
Larger
Smaller
Altering these conditions would increase Q, and thus result in a decrease in the measured cell potential.
Example Question #3 : Cell Potential Under Non Standard Conditions
For the following cell reaction:
2 Al (s) + 3 Mn2+ (aq) -> 2 Al3+ (aq) + 3 Mn (s)
predict if the cell potential Ecell will be larger, or smaller than Eocell for the following conditions: [Al3+] = 1.0 M; [Mn2+] = 5.0 M.
Can not be determined
Identical
Larger
Smaller
Larger
At these concentrations Q will become smaller, and thus log Q will become smaller. This will give rise to a larger cell potential.
Example Question #3 : Cell Potential Under Non Standard Conditions
What is the cell potential of the following cell:
Zn (s) + 2 H+(aq) -> Zn2+ (aq) + H2 (g) Eo = 0.76 V
When the [Zn2+] = 1.0 M; PH2 = 1 atm, and the pH in the cathode is 5.2?
1.32 V
1.59 V
1.80 V
0.90 V
0.45 V
0.45 V
Example Question #4 : Cell Potential Under Non Standard Conditions
Calculate the standard cell potential of the following reaction:
Cd(s) + MnO2 (s) + 4 H+ (aq) + -> Cd2+ (aq) + Mn2+ (aq) + 2 H2O (l)
Given:
MnO2 (s) + 4 H+ (aq) + 2e- -> Mn2+ (aq) + 2 H2O (l) Eo = 1.23 V
Cd2+ (aq) + 2 e- -> Cd (s) Eo = -0.40 V
0.83 V
0.0 V
1.63 V
-0.83 V
-1.63 V
1.63 V
Eocell = Eo cathode - Eoanode
Eocell = 1.23 – (-0.40) = 1.63 V
Example Question #5 : Cell Potential Under Non Standard Conditions
Calculate the standard cell potential of the following reaction:
Zn (s) + Cu2+ (aq) -> Zn2+ (aq) + Cu (s)
Given:
Zn2+(aq)+ 2 e--> Zn (s) Eo = -0.76 V
Cu2+(aq)+ 2 e--> Cu (s) Eo = 0.34 V
1.10 V
-1.10 V
0.0 V
0.42 V
-0.42 V
1.10 V
Eocell = Eo cathode - Eoanode
Eocell = 0.34 – (-0.76) = 1.10 V
Example Question #6 : Cell Potential Under Non Standard Conditions
Calculate the standard cell potential of the following reaction:
Zn (s) + 2 Ag1+ (aq) -> Zn2+ (aq) + 2 Ag (s)
Given:
Zn2+(aq)+ 2 e--> Zn (s) Eo = -0.76 V
Ag1+(aq)+ 1 e--> Ag (s) Eo = 0.80 V
0.04 V
2.36 V
1.56 V
-0.04 V
-1.56 V
1.56 V
Eocell = Eo cathode - Eoanode
Eocell = 0.80 – (-0.76) = 1.56 V
Example Question #2 : Cell Potential Under Non Standard Conditions
Calculate the standard cell potential of the following reaction:
3 F2 (g) + 2 Au (s) -> 6 F- (aq) + 2 Au3+
Given:
F2 (g) + 2 e- -> 2 F- (aq) Eo = 2.87 V
Au3+(aq)+ 3 e--> Au (s) Eo = 1.50 V
-5.61 V
5.61 V
4.37 V
1.37 V
-1.37 V
1.37 V
Eocell = Eo cathode - Eoanode
Eocell = 2.87 – (1.50) = 1.37 V
Example Question #682 : Ap Chemistry
Determine the Ecell for the following reaction at 25 C:
Zn (s) + 2 VO2+ (aq) + 4 H+ -> 2 VO2+ (aq) + Zn2+(aq) + 2 H2O (l)
Given that:
VO2+ (aq) + 2 H+ (aq) + e- -> VO2+(aq) + H2O (l) Eo = 1.00 V
Zn2+ (aq) + 2 e--> Zn (s) Eo = -0.76 V
And
[ VO2+] = 2.0 M; [H+] = 0.50 M; [VO2+] = 1.0 x 10-2M; [Zn2+] = 1.0 x 10-1M
1.89 V
0.95 V
3.71 V
1.76 V
2.41 V
1.89 V
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