3. A galvanic cell was created using the following electrode reactions. Co(s) + 3 en(aq) → [Co(en)3]²*+ (aq) + 2 e Anode half-cell: Cathode half-cell: Co²+, +2e → Co(s) (aq) A. Write the overall cell reaction and the cell notation at standard conditions (concentrations are 1.0 M). B. Given that the standard cell potential (Eºcell) is +0.413 V at 25 °C, determine the formation constant for [Co(en)3]²+ at this temperature. C. Calculate the standard reduction potential (Eºrea) for the cathode half-cell (Co²*/Co) given the standard reduction potential values below. Co³+/Co²+ Co³+/Co Eº red = +1.920 V Eºred = +0.453 V
3. A galvanic cell was created using the following electrode reactions. Co(s) + 3 en(aq) → [Co(en)3]²*+ (aq) + 2 e Anode half-cell: Cathode half-cell: Co²+, +2e → Co(s) (aq) A. Write the overall cell reaction and the cell notation at standard conditions (concentrations are 1.0 M). B. Given that the standard cell potential (Eºcell) is +0.413 V at 25 °C, determine the formation constant for [Co(en)3]²+ at this temperature. C. Calculate the standard reduction potential (Eºrea) for the cathode half-cell (Co²*/Co) given the standard reduction potential values below. Co³+/Co²+ Co³+/Co Eº red = +1.920 V Eºred = +0.453 V
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![3. A galvanic cell was created using the following electrode reactions.
Co(s) + 3 en(aq) → [Co(en)3]²*+ (aq) + 2 e
Anode half-cell:
Cathode half-cell: Co²+,
+2e → Co(s)
(aq)
A. Write the overall cell reaction and the cell notation at standard conditions (concentrations are 1.0
M).
B. Given that the standard cell potential (Eºcell) is +0.413 V at 25 °C, determine the formation constant
for [Co(en)]²+ at this temperature.
C. Calculate the standard reduction potential (Eºrea) for the cathode half-cell (Co²*/Co) given the
standard reduction potential values below.
Co³+/Co²+ Eºred +1.920 V
Co³+/Co
Eºred = +0.453 V
D. Construct the Latimer diagram for Co with these three Co species: Co, Co²+, and Co³+.
E. Calculate the standard oxidation potential (E°ox) for the anode half-cell.](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2F0c6864ed-d5c9-46db-a57c-29b65c0abc90%2F4d78035f-3ff7-42a3-85b9-0064f315f287%2Fqsm38h_processed.png&w=3840&q=75)
Transcribed Image Text:3. A galvanic cell was created using the following electrode reactions.
Co(s) + 3 en(aq) → [Co(en)3]²*+ (aq) + 2 e
Anode half-cell:
Cathode half-cell: Co²+,
+2e → Co(s)
(aq)
A. Write the overall cell reaction and the cell notation at standard conditions (concentrations are 1.0
M).
B. Given that the standard cell potential (Eºcell) is +0.413 V at 25 °C, determine the formation constant
for [Co(en)]²+ at this temperature.
C. Calculate the standard reduction potential (Eºrea) for the cathode half-cell (Co²*/Co) given the
standard reduction potential values below.
Co³+/Co²+ Eºred +1.920 V
Co³+/Co
Eºred = +0.453 V
D. Construct the Latimer diagram for Co with these three Co species: Co, Co²+, and Co³+.
E. Calculate the standard oxidation potential (E°ox) for the anode half-cell.
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