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-Equation A g ( ) + e A g ( ) + a q s F e ( ) + 2 e F e ( ) 2 + a q s
Standard Electrode Potential, 𝐸 (V) + 0 . 7 9 9 6 0 . 4 4 7

Q2:

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

Half-equation S n ( ) + 2 e S n ( ) 2 + a q s C u ( ) + e C u ( ) 2 + + a q a q
Standard electrode potential, 𝐸 (V) 0 . 1 3 7 5 + 0 . 1 5 3

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?

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