The electrolysis of BiO^+ produces pure bismuth. How long...

The electrolysis of $\mathrm{BiO}^{+}$ produces pure bismuth. How long would it take to produce $10.0 \mathrm{~g} \mathrm{Bi}$ by the electrolysis of a $\mathrm{BiO}^{+}$ solution using a current of $25.0 \mathrm{~A}$ ?

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Key Concepts

Faraday's Laws of Electrolysis

Faraday's laws provide the fundamental relationship between the amount of substance deposited at an electrode and the total charge passed through the electrolyte. These laws allow one to calculate the mass of a substance produced during an electrochemical reaction from the charge, taking into account the molar mass and the number of electrons involved in the reaction.

Electric Current and Charge

Electric current is the rate at which charge flows, and it is directly related to the total charge passed through an electrolysis cell over time. This relationship is expressed by the formula Q = I × t, where Q is the total charge, I is the current, and t is the time, allowing one to determine the time required to produce a desired quantity of a substance.

Stoichiometric Calculations in Electrolysis

Stoichiometry in electrolysis involves converting between the mass of a substance and the number of moles of electrons needed for its formation. By using the substance's molar mass and the stoichiometric coefficients from the balanced redox reaction, one can relate the amount of substance formed to the charge required, bridging fundamental concepts of chemistry with electrochemical processes.

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