We are asked to calculate for the Ecell for the reaction.
Cu(s) | Cu2+(0.017 M) || Ag(s), (Ag+ = 0.18M)
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 Ecell using the Nernst Equation.
What is E of the following cell reaction at 25°C? E°cell = 0.460 V.
Cu(s) | Cu2+(0.017 M) || Ag(s), (Ag+ = 0.18 M)
B) 0.282 V
C) 0.460 V
D) 0.490 V
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