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Part C. Effect of Concentration on Cell Potentials • Ecall for the Cu(s). Cu2+||Ag*, Ag(s) system:...
Compare the potentials between the Ag/Ag+ and Cu/Cu2+ half cells before and after adding excess NH3...
Compare the potentials between the Ag/Ag+ and Cu/Cu2+ half cells before and after adding excess NH3 to the Cu/Cu2+ half cell. Did the potential increase or decrease? Explain the result in terms of the Nernst equation.
Identify the complete redox reaction for a CulCu2+||Ag+Ag cell. A. Cu(s) + Ag(s) Cu2+ (aq) +...
Identify the complete redox reaction for a CulCu2+||Ag+Ag cell. A. Cu(s) + Ag(s) Cu2+ (aq) + Ag+ (aq) B. Cu(s) + Ag+ (aq) + Cu2+ (aq) + Ag(s) c. Cu(s) + 2 Ag+ (aq) (aq) + 2 Ag(s) D. Cu²+ (aq) + 2 Ag(s) + Cu(s) + 2 Ag+ (aq) → Cu2+
11. Write the balanced redox reaction corresponding to the following cell diagram: Cu(s) / Cu2+ ( 1M) || Ag+ (1M) /...
11. Write the balanced redox reaction corresponding to the following cell diagram: Cu(s) / Cu2+ ( 1M) || Ag+ (1M) / Ag(s)
Use the table of Standdard Reduction Potentials and the Nernst Equation to calculate the concentration of...
Use the table of Standdard Reduction Potentials and the Nernst
Equation to calculate the concentration of Cu2+ present in the
Cu/Cu2+ half-cell after the addition NH3 (aq) while it was coupled
with
a) Zn/Zn2+
b) Ag/Ag+
Table 2 has your measured voltages for these cells. SHOW YOUR
SETUP OF THE NERST EQUATION WITH ALL VARIABLES FILLED IN. SHOW THE
CALCULATED [Cu2+] CONCENTRATION.
Table 2:
METAL
Mg
Ag
Ni
Zn
Pb
Cu
1.230 V
0.642 V
0.030 V
0.648 V
0.256...
During part B of your lab, you measured electrochemical cell potentials with a Cu2+/Cu couple as...
During part B of your lab, you measured electrochemical cell potentials with a Cu2+/Cu couple as the anode. Predict the results you would observe if Ag+/Ag were the anode. half-cell predicted potential difference in V Cu2+/Cu Ag+/Ag Pb2+/Pb Zn2+/Zn
During part B of your lab, you measured electrochemical cell potentials with a Cu2+/Cu couple as...
During part B of your lab, you measured electrochemical cell potentials with a Cu2+/Cu couple as the anode. Predict the results you would observe if Ag+/Ag were the anode. half-cell predicted potential difference in V Cu2+/Cu Ag+/Ag Pb2+/Pb Zn2+/Zn
Calculate the E°cell for the following reaction: Cu2+ (aq) + Ni (s) → Cu (s)...
Calculate the E°cell for the following reaction: Cu2+ (aq) + Ni (s) → Cu (s) + Ni2+ (aq) A) (-0.59 ± 0.01) V B) (-0.09 ± 0.01) V C) (0.59 ± 0.01) V D) (0.09 ± 0.01) V --------------------------------------------------------------------------------------------------------- What is the proper line notation for the following reaction? Cu (s) + 2Ag+ (aq) → Cu2+ (aq) + 2Ag (s) A) Cu2+ | Cu || Ag | Ag+ B) Ag+ | Ag || Cu | Cu2+ C) Cu |...
Suppose a concentration cell of: Cu(s) | Cu2+(dilute) || Cu2+(concentrated)| Cu(s) is made with the following...
Suppose a concentration cell of: Cu(s) | Cu2+(dilute) || Cu2+(concentrated)| Cu(s) is made with the following concentrations: Dilute: Cu2+ = 2.5 x 10-4 Concentrated: Cu2+ = 5.0 x 10-2 What will be the cell potential of the cell? 0.084 V 0.0 V 0.030 V 0 0.013 V
cell A voltaic cell employs the following redox reaction: Cu(s) + 2 Ag+ (aq) – Cu...
cell A voltaic cell employs the following redox reaction: Cu(s) + 2 Ag+ (aq) – Cu 2+ (aq) + 2 Ag(s) The E° for the reaction is +0.46 V. The initial (nonstandard) conditions are: [Ag +] = 0.025M; [Cu 2+] = 2.0 M Part a. Write the half-reaction that occurs at the anode. Part b. Write the half-reaction that occurs at the cathode. Part c. How many electrons are transferred in this reaction? Part d. What is the cell potential,...
Calculate the E°cell for the following reaction: Cu2+ (aq) + Ni (s) → Cu (s)...
Calculate the E°cell for the following reaction: Cu2+ (aq) + Ni (s) → Cu (s) + Ni2+ (aq) A) (-0.59 ± 0.01) V B) (-0.09 ± 0.01) V C) (0.59 ± 0.01) V D) (0.09 ± 0.01) V --------------------------------------------------------------------------------------------------------- What is the proper line notation for the following reaction? Cu (s) + 2Ag+ (aq) → Cu2+ (aq) + 2Ag (s) A) Cu2+ | Cu || Ag | Ag+ B) Ag+ | Ag || Cu | Cu2+ C) Cu |...
Identify the complete redox reaction for a CulCu2+||Ag+Ag cell. A. Cu(s) + Ag(s) Cu2+ (aq) + Ag+ (aq) B. Cu(s) + Ag+ (aq) + Cu2+ (aq) + Ag(s) c. Cu(s) + 2 Ag+ (aq) (aq) + 2 Ag(s) D. Cu²+ (aq) + 2 Ag(s) + Cu(s) + 2 Ag+ (aq) → Cu2+
11. Write the balanced redox reaction corresponding to the following cell diagram: Cu(s) / Cu2+ ( 1M) || Ag+ (1M) / Ag(s)
Use the table of Standdard Reduction Potentials and the Nernst
Equation to calculate the concentration of Cu2+ present in the
Cu/Cu2+ half-cell after the addition NH3 (aq) while it was coupled
with
a) Zn/Zn2+
b) Ag/Ag+
Table 2 has your measured voltages for these cells. SHOW YOUR
SETUP OF THE NERST EQUATION WITH ALL VARIABLES FILLED IN. SHOW THE
CALCULATED [Cu2+] CONCENTRATION.
Table 2:
METAL
Mg
Ag
Ni
Zn
Pb
Cu
1.230 V
0.642 V
0.030 V
0.648 V
0.256...
Suppose a concentration cell of: Cu(s) | Cu2+(dilute) || Cu2+(concentrated)| Cu(s) is made with the following concentrations: Dilute: Cu2+ = 2.5 x 10-4 Concentrated: Cu2+ = 5.0 x 10-2 What will be the cell potential of the cell? 0.084 V 0.0 V 0.030 V 0 0.013 V
cell A voltaic cell employs the following redox reaction: Cu(s) + 2 Ag+ (aq) – Cu 2+ (aq) + 2 Ag(s) The E° for the reaction is +0.46 V. The initial (nonstandard) conditions are: [Ag +] = 0.025M; [Cu 2+] = 2.0 M Part a. Write the half-reaction that occurs at the anode. Part b. Write the half-reaction that occurs at the cathode. Part c. How many electrons are transferred in this reaction? Part d. What is the cell potential,...
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