A sample of 1.0 mol dm-3 copper (II) sulfate solution was electrolyzed for 1 hour using copper...


A sample of 1.0 mol{eq}\cdot {/eq}dm{eq}^{-3} {/eq} copper (II) sulfate solution was electrolyzed for 1 hour using copper electrodes. Which change would have caused the largest increase in the amount of copper deposited?

a. increasing the concentration of the copper (II) sulfate to 1.1 mol{eq}\cdot {/eq}dm{eq}^{-3} {/eq}

b. increasing the current by 10%

c. increasing the surface area of the electrodes by 10%

d. changing the electrodes from copper to graphite

Faraday's First Law:

With electricity, a nonspontaneous chemical reaction is conducted in an electrolytic cell. The amount of required metal deposited can be calculated as:

{eq}\rm mass\,of\,the\,metal= \dfrac{E\times I \times time}{F} {/eq}

E=equivalent weight of the metal.

I=current in amp

F=96500 Coulombs

Answer and Explanation: 1

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The given data is:

Time = 1 hour

{eq}\rm Cu^{2+} = 1.0 M {/eq}

The reaction that takes place at the cathode is:

{eq}\rm Cu^{2+}(aq) \to...

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Electrolysis: Definition, Types & Uses


Chapter 20 / Lesson 5

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