1. A voltaic cell consists of a copper electrode in a solution of copper(II) ion

Question

1. A voltaic cell consists of a copper electrode in a solution of copper(II) ions with unknown concentration, and a palladium electrode in a 0.1 M solution of palladium(II) ions. The palladium electrode is the cathode and its reduction potential is 0.951 V, the Cu electrode is the anode.

(a) Write the half-reaction that occurs at the anode and the cathode, as well as the overall cell reaction.

(b) What is the concentration of Cu2+ ions in the anode if the cell potential is 0.584 V? Speculate why this is not a very accurate measurement to determine the Cu2+ concentration.

(c) What is the equilibrium constant (Keq) for this reaction?

2. You have built the electrolytic cell below.

a) Write the chemical equation for the anodic and cathodic processes. What is the overall reaction?

b) How many moles/grams of oxygen and hydrogen are produced after 5 min of electrolysis at a current of 0.23 A? What is the volume of the gases at room temperature and atmospheric pressure (assume ideal gas law). What is the total number of electrons that passed the electrode/electrolyte interface?

3. What is the current measured in a circuit involving the half cell reaction Sn+4 + 2e- %u2192 Sn+2 which is occurring at a rate of 4.2 x 10-3 mole/hr?

4. Calculate the potential in the following cell

Zn|Zn2+(1.00M)|| Cu2+(1.00M) |Cu

a) right at the beginning when you start using this voltaic cell,

b) when 50% of the Cu2+ ions have been consumed,

c) when 99% of the Cu2+ ions have been consumed, and

d) when 99.99% of the Cu2+ ions have been consumed.

Keep in mind that both, the Zn2+ and the Cu2+ concentrations are changing.

Picture of th circut for question 2.

Explanation / Answer

4.

Zn2+ + 2e-----> Zn   -0.7628V

Cu2+ + 2e- ---

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