In this worksheet, we will practice converting the potential of an electrochemical cell to the change in free energy and equilibrium constant.

Q1:

Using the standard electrode potentials in the table, calculate to 2 significant figures the equilibrium constant at for the following reaction.

Half-Equation

Standard Electrode Potential, (V)

+0.7996

A

B

C

D

E

Q2:

Using the standard electrode potentials in the table below, calculate to 2 significant figures the equilibrium constant at for a galvanic cell with the following overall reaction.

Half-Equation

Standard Electrode Potential, (V)

A

B

C3.5

D

E

Q3:

Calculate, to 3 significant figures, the value of the reaction quotient for the cell diagram shown.

Q4:

What is the cell potential of the concentration cell shown?

Q5:

A concentration cell has the following cell diagram.

The cell potential for this cell, , is 0.10 V at 298 K.
Calculate, to 2 significant figures, the value of the reaction quotient, .

A7.0

B

C

D

E49

Q6:

For the concentration cell described by the cell diagram shown,
the reaction quotient, , is . Calculate, to 2 significant figures,
the concentration of at the anode of the cell.

A
M

B
M

C
M

D
M

E
M

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