Worksheet: Gibbs Energies for Electrochemical Cells

In this worksheet, we will practice calculating the standard change in Gibbs free energy from the cell potential of an electrochemical cell.

Q1:

Using the standard electrode potentials in the table, calculate to 3 significant figures the standard free energy change at 25C for the reaction shown. 2Ag()+Fe()2Ag()+Fe()+2+aqssaq

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

Q2:

What is the standard free energy change for the following reaction at 25C?

Sn()+2Cu()Sn()+2Cu()saqaqaq2+2++

Half-EquationSn()+2eSn()2+aqsCu()+eCu()2++aqaq
Standard Electrode Potential, 𝐸 (V)0.1375+0.153

Q3:

For a galvanic cell with Δ𝐺 of 15 kJ/mol, where 𝑛=2, what is the standard cell potential?

Q4:

For a galvanic cell with Δ𝐺 of 30 kJ/mol, where 𝑛=3, what is the standard cell potential?

Q5:

For a standard cell potential of 0.000 V, where 𝑛=2, what is the Δ𝐺 for the cell?

Q6:

In an electrochemical cell, the transfer of 2 electrons from 1 mol of reductant to 1 mol of oxidant produces a standard cell potential of +0.434 V. Calculate the value of Δ𝐺 for this cell.

Q7:

For a standard cell potential of 2.439 V where 𝑛=1, what is the Δ𝐺 for the cell?

Nagwa uses cookies to ensure you get the best experience on our website. Learn more about our Privacy Policy.