Worksheet: Cell Potentials and Equilibrium Constants

In this worksheet, we will practice converting the potential of an electrochemical cell to the change in free energy and equilibrium constant.

Q1:

Using the standard electrode potentials in the table, calculate to 2 significant figures the equilibrium constant at 25C for the following reaction. 2Ag()+Fe()2Ag()+Fe()+2+aqssaq

Half-EquationAg()+eAg()+aqsFe()+2eFe()2+aqs
Standard Electrode Potential, 𝐸 (V)+0.79960.447
  • A1.4×10
  • B8.4×10
  • C2.0×10
  • D7.2×10
  • E1.2×10

Q2:

Using the standard electrode potentials in the table below, calculate to 2 significant figures the equilibrium constant at 25C for a galvanic cell with the following overall reaction. Sn()+2Cu()Sn()+2Cu()saqaqaq2+2++

Half-EquationSn()+2eSn()2+aqsCu()+eCu()2++aqaq
Standard Electrode Potential, 𝐸 (V)0.1375+0.153
  • A8.2×10
  • B6.6×10
  • C3.5
  • D0.035×10
  • E6.4×10

Q3:

Calculate, to 3 significant figures, the value of the reaction quotient for the cell diagram shown. Al()Al(,0.150M)Cu(,0.0250M)Cu()saqaqs||3+2+

Q4:

What is the cell potential of the concentration cell shown? Zn()Zn(,0.10M)Zn(,0.50M)Zn()saqaqs||2+2+

Q5:

A concentration cell has the following cell diagram. Zn()Zn()Zn()Zn()saqaqs||2+2+

The cell potential for this cell, 𝐸cell, is 0.10 V at 298 K. Calculate, to 2 significant figures, the value of the reaction quotient, 𝑄.

  • A7.0
  • B2.4×10
  • C4.1×10
  • D2.0×10
  • E49

Q6:

For the concentration cell described by the cell diagram shown, the reaction quotient, 𝑄, is 4.2×10. Calculate, to 2 significant figures, the concentration of Zn2+ at the anode of the cell. Zn()Zn()Zn(,0.50M)Zn()saqaqs||2+2+

  • A4.1×10 M
  • B8.4×10 M
  • C2.1×10 M
  • D1.0×10 M
  • E1.2×10 M

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