We are asked to calculate for the cell potential (Ecell) for the voltaic cell below:
Zn(s), [Zn2+] = 4.50M] || Cu(s), [Cu2+] = 0.0120M
We can rewrite the cell notation as:
Zn(s) | Zn2+, (4.50 M) || Cu2+, (0.0120M) | Cu(s)
Recall that the Nernst Equation relates the concentrations of compounds and cell potential.
Ecell = cell potential under non-standard conditions
E°cell = standard cell potential
n = mole e- transferred
Q = reaction quotient = products/reactants
We're going to calculate for the Ecell using the following steps:
Step 1: Identify the anode and the cathode in the reaction and write the overall reaction
Step 2: Calculate the cell potential of the reaction.
Step 3: Calculate Ecell using the Nernst Equation.
Given the voltaic cell below, find the cell potential.
Zn(s), [Zn2+]=4.50M] || Cu(s), [Cu2+]=0.0120M
Cu2+(aq) + 2e– ⇌ Cu(s) E° = 0.34 V
Zn2+(aq) + 2e– ⇌ Zn(s) E° = -0.76 V
A) 1.23 V
B) 1.10 V
C) 1.18 V
D) 1.02 V
E) 1.08 V
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