2. Consider a concentration cell which used the following half-reaction at 273 K. Co2*(aq) + 2e- → Co(s) E° = -0.28 V KNO3 salt bridge Cobalt Electrode Cobalt Electrode 1.50 M Co2+ 0.0025 М Со2+ a. Label the anode, cathode, current, anion flow, and cation flow. b. Write a balanced equation for the cell reaction. Calculate the cell potential. С.
2. Consider a concentration cell which used the following half-reaction at 273 K. Co2*(aq) + 2e- → Co(s) E° = -0.28 V KNO3 salt bridge Cobalt Electrode Cobalt Electrode 1.50 M Co2+ 0.0025 М Со2+ a. Label the anode, cathode, current, anion flow, and cation flow. b. Write a balanced equation for the cell reaction. Calculate the cell potential. С.
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Chapter1: Chemical Foundations
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![2. Consider a concentration cell which used the following half-reaction at 273 K.
Со2*(ад) + 2е- > Со(s)
E° = -0.28 V
KNO3 salt bridge
Cobalt Electrode
Cobalt Electrode
1.50 М Со2+
0.0025 М Со2+
a. Label the anode, cathode, current, anion flow, and cation flow.
b. Write a balanced equation for the cell reaction.
c. Calculate the cell potential.
d. Calculate the equilibrium [Co2+] at the anode and cathode.](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2F6aee40a3-e3f8-4130-be7a-2391988c5efd%2F4607dc71-c1dd-400e-8478-3cae73cba217%2F5hfbvcr_processed.png&w=3840&q=75)
Transcribed Image Text:2. Consider a concentration cell which used the following half-reaction at 273 K.
Со2*(ад) + 2е- > Со(s)
E° = -0.28 V
KNO3 salt bridge
Cobalt Electrode
Cobalt Electrode
1.50 М Со2+
0.0025 М Со2+
a. Label the anode, cathode, current, anion flow, and cation flow.
b. Write a balanced equation for the cell reaction.
c. Calculate the cell potential.
d. Calculate the equilibrium [Co2+] at the anode and cathode.
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