Lesson: Cell Potentials and Equilibrium Constants

Chemistry

In this lesson, we will learn how to convert the potential of an electrochemical cell to the change in free energy and equilibrium constant.

Sample Question Videos

  • 09:36

Worksheet

Q1:

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

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

Q2:

Using the standard electrode potentials in the table below, calculate to 2 significant figures the equilibrium constant at 25∘C 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

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+
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