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In this lesson, we will learn how to use the Nernst equation to calculate reduction potentials under nonstandard concentrations.

Q1:

Using the standard electrode potentials shown in the table, calculate to 2 decimal places the cell potential at 298.15 K for the cell with the overall reaction:

Q2:

Calculate to 3 significant figures the cell potential for the following reaction at 298 K?

Q3:

Using the standard electrode potentials shown in the table, calculate to 2 significant figures the equilibrium constant at 373 K for the reaction:

Q4:

Calculate to 2 significant figures the equilibrium constant at 2 5 ∘ C for the reaction:

Note that each standard electrode potential is expressed per mole of the half-reaction shown in the table.

Q5:

Q6:

The half-cells of a galvanic cell consist of an aluminum electrode in a 0.0150 M aluminum nitrate solution and a nickel electrode in a 0.250 M nickel(II) nitrate solution. Using the standard electrode potentials shown in the table, calculate to 2 decimal places the cell potential for the galvanic cell at 298.15 K. Note that standard electrode potentials are measured using 1.00 M solutions of the reacting ions.

Q7:

In the half-cells of an electrochemical cell, 1.00 M aqueous bromide ions are oxidized to 0.110 M bromine and 0.0230 M aluminum ions are reduced to aluminum metal. Using the standard electrode potentials shown in the table, calculate to 3 decimal places the cell potential for the cell at 298.15 K. Note that standard electrode potentials are measured using 1.00 M solutions of the reacting ions.

Q8:

A battery is dead when it has no cell potential. Consider a battery with the overall reaction: The standard electrode potentials for the half-cells in this battery are given in the table.

To 2 significant figures, what is the value of 𝑄 when this battery is dead at 298.15 K?

If a particular dead battery is found to have [ C u ] 2 + = 0.11 M, what is the concentration of silver ions?

Q9:

Using the standard electrode potential data in the table, calculate the standard cell potential for the following reaction at 298 K.

Q10:

Using the standard electrode potentials shown in the table, calculate to 2 significant figures the equilibrium constant at 298.15 K for the reaction:

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