Cell Potential Under Non-standard Conditions - AP Chemistry
Card 0 of 117
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
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
Eocell = Eo cathode - Eoanode
Eocell = 0.80 – (-0.76) = 1.56 V
Eocell = Eo cathode - Eoanode
Eocell = 0.80 – (-0.76) = 1.56 V
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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
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
Eocell = Eo cathode - Eoanode
Eocell = 2.87 – (1.50) = 1.37 V
Eocell = Eo cathode - Eoanode
Eocell = 2.87 – (1.50) = 1.37 V
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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?
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?
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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
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
Eocell = Eo cathode - Eoanode
Eocell = 1.23 – (-0.40) = 1.63 V
Eocell = Eo cathode - Eoanode
Eocell = 1.23 – (-0.40) = 1.63 V
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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
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
Eocell = Eo cathode - Eoanode
Eocell = 0.34 – (-0.76) = 1.10 V
Eocell = Eo cathode - Eoanode
Eocell = 0.34 – (-0.76) = 1.10 V
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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?
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?
All of these changes would change Q and thus change the measured cell potential.
All of these changes would change Q and thus change the measured cell potential.
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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.
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.
Altering these conditions would increase Q, and thus result in a decrease in the measured cell potential.
Altering these conditions would increase Q, and thus result in a decrease in the measured cell potential.
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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
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
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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.
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.
At these concentrations Q will become smaller, and thus log Q will become smaller. This will give rise to a larger cell potential.
At these concentrations Q will become smaller, and thus log Q will become smaller. This will give rise to a larger cell potential.
Compare your answer with the correct one above
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?
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?
All of these changes would change Q and thus change the measured cell potential.
All of these changes would change Q and thus change the measured cell potential.
Compare your answer with the correct one above
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.
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.
Altering these conditions would increase Q, and thus result in a decrease in the measured cell potential.
Altering these conditions would increase Q, and thus result in a decrease in the measured cell potential.
Compare your answer with the correct one above
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
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
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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.
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.
At these concentrations Q will become smaller, and thus log Q will become smaller. This will give rise to a larger cell potential.
At these concentrations Q will become smaller, and thus log Q will become smaller. This will give rise to a larger cell potential.
Compare your answer with the correct one above
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?
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?
Compare your answer with the correct one above
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
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
Eocell = Eo cathode - Eoanode
Eocell = 1.23 – (-0.40) = 1.63 V
Eocell = Eo cathode - Eoanode
Eocell = 1.23 – (-0.40) = 1.63 V
Compare your answer with the correct one above
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
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
Eocell = Eo cathode - Eoanode
Eocell = 0.34 – (-0.76) = 1.10 V
Eocell = Eo cathode - Eoanode
Eocell = 0.34 – (-0.76) = 1.10 V
Compare your answer with the correct one above
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
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
Eocell = Eo cathode - Eoanode
Eocell = 0.80 – (-0.76) = 1.56 V
Eocell = Eo cathode - Eoanode
Eocell = 0.80 – (-0.76) = 1.56 V
Compare your answer with the correct one above
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
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
Eocell = Eo cathode - Eoanode
Eocell = 2.87 – (1.50) = 1.37 V
Eocell = Eo cathode - Eoanode
Eocell = 2.87 – (1.50) = 1.37 V
Compare your answer with the correct one above
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
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
Eocell = Eo cathode - Eoanode
Eocell = 0.80 – (-0.76) = 1.56 V
Eocell = Eo cathode - Eoanode
Eocell = 0.80 – (-0.76) = 1.56 V
Compare your answer with the correct one above
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
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
Eocell = Eo cathode - Eoanode
Eocell = 2.87 – (1.50) = 1.37 V
Eocell = Eo cathode - Eoanode
Eocell = 2.87 – (1.50) = 1.37 V
Compare your answer with the correct one above