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Electrolysis and Faraday's Law Practice Test
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Q1
An aqueous solution containing $\text{Cu}^{2+}$ is electrolyzed with an inert cathode. A total charge of $1.93\times 10^4\ \text{C}$ passes through the circuit. Copper metal plates onto the cathode according to $\text{Cu}^{2+}+2e^-\rightarrow \text{Cu}(s)$. Assuming 100% current efficiency, how many moles of $\text{Cu}(s)$ are produced?
An aqueous solution containing $\text{Cu}^{2+}$ is electrolyzed with an inert cathode. A total charge of $1.93\times 10^4\ \text{C}$ passes through the circuit. Copper metal plates onto the cathode according to $\text{Cu}^{2+}+2e^-\rightarrow \text{Cu}(s)$. Assuming 100% current efficiency, how many moles of $\text{Cu}(s)$ are produced?