What is the hourly production rate of chlorine gas (in kg)...

What is the hourly production rate of chlorine gas (in kg) from an electrolytic cell using aqueous $\mathrm{NaCl}$ electrolyte and carrying a current of $1.500 \times 10^{3} \mathrm{~A}$ ?
The anode efficiency for the oxidation of $\mathrm{Cl}^{-}$ is $93.0$ percent.

Key Concepts

Relationship between Charge, Current, and Time

The fundamental relationship in electrolysis is Q = I × t, where Q is the total electric charge, I is the current, and t is the time. This equation is essential for determining the total number of electrons that participate in the reaction, serving as the basis for further stoichiometric calculations.

Stoichiometry of Electrochemical Reactions

Stoichiometry in electrochemical reactions involves using the balanced chemical equation to relate the electrons transferred to the number of moles of reactants consumed or products formed. This concept is vital for converting the electron charge into the corresponding mass of product, such as chlorine gas in an electrolytic cell.

Current Efficiency

Current efficiency, often referred to as electrolysis efficiency, measures the proportion of the electric charge that contributes effectively to the desired chemical reaction. It accounts for losses due to side reactions or other inefficiencies, thereby adjusting the theoretical yield to more practical figures.

Faraday's Law of Electrolysis

Faraday's law connects the quantitative amount of substance transformed at an electrode to the total electric charge passed through the system. This principle helps in calculating the number of moles of electrons involved in the electrolysis process, which is then used to determine the mass of a product formed based on the reaction stoichiometry.

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