We are asked to calculate for the Ecell for the reaction.
Mg(s) I Mg2+(aq)(0.15 M) II Au+(aq)(0.3 M) I Au(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.
What is the Ecell for Mg(s) I Mg2+(aq)(0.15 M) II Au+(aq)(0.3 M) I Au(s) ? Assume that the number of electrons transferred in the reaction is n = 2.
Mg2+ + 2e- → Mg E°red = -2.36 V
Au+ + e- → Au E°red = +1.69 V
1. 4.04 V
2. 4.08 V
3. 3.2 x 10-2 V
4. 4.03 V
5. 4.01 V
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