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? 2Ag()+Fe()2Ag()+Fe()+2+aqssaq

Half-EquationAg()+eAg()+aqsFe()+2eFe()2+aqs
Standard Electrode Potential, 𝐸 (V)+0.79960.447

Q2:

A galvanic cell consists of a Mg electrode in 1 MMg(NO)32 solution and a Ag electrode in 1 MAgNO3 solution. What is the standard cell potential?

Half-Equation Mg()+2eMg()2+aqsAg()+eAg()+aqs
Standard Electrode Potential, 𝐸 (V)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 Au3+/Au and Ni2+/Ni half-cells.

Half-EquationAu()+3eAu()3+aqsNi()+2eNi()+aqs
Standard Electrode Potential, 𝐸 (V)+1.4980.257
  • A1.241 V
  • B1.755 V
  • C1.755 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. Sn()+2Cu()Sn()+2Cu()saqaqaq2+2++

Half-Equation Sn()+2eSn()2+aqsCu()+eCu()2++aqaq
Standard Electrode Potential, 𝐸 (V)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. Cd()|Cd(,0.10M)Ni(,0.50M)|Ni()saqaqs2+2+

Half-EquationCd()+2eCd()2+aqsNi()+2eNi()2+aqs
Standard Electrode Potential, 𝐸()V0.40300.257
  • 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 LaO23 to La metal.

Half-EquationCa()+2eCa()2+aqsAl()+3eAl()3+aqsFe()+2eFe()2+aqsLa()+3eLa()3+aqs
Standard Electrode Potential, 𝐸 (V)2.8681.6620.4472.52
  • AAl only
  • BCa only
  • CFe only
  • DAl and Fe
  • ECa and Al

Q7:

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

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

Based on the cell potentials, which of the two complexes, [Co(HO)]262+ and [Co(NH)]362+, can be oxidized to the corresponding cobalt(III) complex by oxygen? Assume that all reactions take place under standard conditions.

  • A[Co(NH)]362+ and [Co(HO)]262+
  • B[Co(HO)]262+ but not [Co(NH)]362+
  • C[Co(NH)]362+ but not [Co(HO)]262+
  • DNeither [Co(HO)]262+ nor [Co(NH)]362+
  • EMore information is needed.

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