# Worksheet: Electrochemical Cell Potential

In this worksheet, we will practice calculating the potential of an electrochemical cell from the half-cell potentials of the anode and cathode.

Q1:

What is the standard electrode potential for the galvanic cell with the following overall reaction?

Half-Equation Standard Electrode Potential, 𝐸⦵ (V) Ag()+eAg()+–aqs Fe()+2eFe()2+–aqs +0.7996 −0.447

Q2:

A galvanic cell consists of a electrode in 1 M solution and a electrode in 1 M solution. What is the standard cell potential?

Half-Equation Standard Electrode Potential, 𝐸⦵ (V) Mg()+2eMg()2+–aqs Ag()+eAg()+–aqs −2.372 +0.7996

Q3:

Using the standard electrode potentials in the table below, calculate the standard cell potential for a galvanic cell consisting of / and / half-cells.

Half-Equation Standard Electrode Potential, 𝐸⦵ (V) Au()+3eAu()3+–aqs Ni()+2eNi()+–aqs +1.498 −0.257
• A V
• B1.755 V
• C V
• D1.241 V

Q4:

Using the standard electrode potentials in the table below, calculate the standard cell potential for a galvanic cell with the following overall reaction.

Half-Equation Standard Electrode Potential, 𝐸⦵ (V) Sn()+2eSn()2+–aqs Cu()+eCu()2+–+aqaq −0.1375 +0.153

Q5:

Using the standard electrode potentials shown in the table, calculate, to 3 decimal places, the cell potential for the following electrochemical cell.

Half-Equation Standard Electrode Potential, 𝐸()⦵V Cd()+2eCd()2+–aqs Ni()+2eNi()2+–aqs −0.4030 −0.257
• A0.167 V
• B0.146 V
• C0.164 V
• D0.155 V
• E0.125 V

Q6:

Using the standard electrode potentials shown in the table, determine which of the following metals are capable of reducing to metal.

 Half-Equation Standard Electrode Potential, 𝐸⦵ (V) Ca()+2eCa()2+–aqs Al()+3eAl()3+–aqs Fe()+2eFe()2+–aqs La()+3eLa()3+–aqs −2.868 −1.662 −0.447 −2.52
• A only
• B only
• C only
• D and
• E and

Q7:

The standard reduction potentials for oxygen gas and two cobalt(III) complexes are shown in the table.

 Half-Equation Standard Electrode Potential, 𝐸()⦵V O()+4H()+4e2HO()2+–2gaql [Co(HO)]()+e[Co(HO)]()263+–262+aqaq [Co(NH)]()+e[Co(NH)]()363+–362+aqaq +1.229 +1.8 +0.1

Based on the cell potentials, which of the two complexes, and , can be oxidized to the corresponding cobalt(III) complex by oxygen? Assume that all reactions take place under standard conditions.

• A and
• B but not
• C but not
• DNeither nor