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In this lesson, we will learn how to calculate the potential of an electrochemical cell from the half-cell potentials of the anode and cathode.

Q1:

A galvanic cell consists of a M g electrode in 1 Mβ M g ( N O ) 3 2 solution and a A g electrode in 1 Mβ A g N O 3 solution. What is the standard cell potential?

Q2:

Using the standard electrode potentials shown in the table, determine which of the following metals are capable of reducing L a O 2 3 to L a metal.

Q3:

The standard reduction potentials for oxygen gas and two cobalt(III) complexes are shown below:

Based on the cell potentials, which of the two complexes, [ C o ( H O ) ] 2 6 2 + and [ C o ( N H ) ] 3 6 2 + , can be oxidized to the corresponding cobalt(III) complex by oxygen? Assume that all reactions take place under standard conditions.

Q4:

Using the standard electrode potentials shown in the table, calculate to 3 decimal places the cell potential for the electrochemical cell:

Q5:

Using the standard electrode potentials in the table below, calculate the standard cell potential for a galvanic cell with the overall reaction:

Q6:

What is the standard electrode potential for the galvanic cell with the following overall reaction?

Q7:

Using the standard electrode potentials in the table below, calculate the standard cell potential for a galvanic cell consisting of A u 3 + / A u and N i 2 + / N i half-cells.

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