Problem: An electrochemical cell has the following half cell reactions: Cu2+(aq) +2e- → Cu(s)          E°1/2 = +0.34 Zn2+(aq) + 2e- → Zn(s)          E°1/2 = -0.76 If the cell operates with the Cu electrode as the cathode and the Zn as the anode, What is the cell potential when the [Cu2+] = 0.001M and the [Zn2+] = 0.1M? A) 1.159V B) -1.159 V C) +0.479 V D) -0.479 V E) +1.041 V

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Problem Details

An electrochemical cell has the following half cell reactions:
Cu2+(aq) +2e- → Cu(s)          E°1/2 = +0.34

Zn2+(aq) + 2e- → Zn(s)          E°1/2 = -0.76

If the cell operates with the Cu electrode as the cathode and the Zn as the anode, What is the cell potential when the [Cu2+] = 0.001M and the [Zn2+] = 0.1M?


A) 1.159V
B) -1.159 V
C) +0.479 V
D) -0.479 V
E) +1.041 V

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