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General Chemistry

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Change in Electrode Mass of Copper Concentration Cell

CHEM-D$SO1N

Consider a concentration cell at $25°C$ using the following half reaction:

$$\textrm{Cu}^{2+}(aq) + 2e^- \rightarrow \textrm{Cu}(s)$$

Two copper electrodes, each weighing $20.0 \textrm{ g}$, and containing $1.00 \textrm{ L}$ of $0.500 \textrm{ M Cu}^{2+}$ solution and $1.00 \textrm{ L}$ of $0.150 \textrm{ M Cu}^{2+}$ solution, respectively, are assembled with two beakers, wire, and a salt bridge.

What will the mass of the electrode at the anode be when the cell potential is $0.00750 \textrm{ V}$?

A

$5.24 \textrm{ g}$

B

$11.87 \textrm{ g}$

C

$14.8 \textrm{ g}$

D

$20.0 \textrm{ g}$

E

$25.2 \textrm{ g}$