One of the few industrial-scale processes that produce...

One of the few industrial-scale processes that produce organic compounds electrochemically is used by the Monsanto Company to produce 1,4 -dicyanobutane. The reduction reaction is $$2 \mathrm{CH}_{2}=\mathrm{CHCN}+2 \mathrm{H}^{+}+2 \mathrm{e}^{-} \longrightarrow \mathrm{NC}-\left(\mathrm{CH}_{2}\right)_{4}-\mathrm{CN}$$ The $\mathrm{NC}-\left(\mathrm{CH}_{2}\right)_{4}-\mathrm{CN}$ is then chemically reduced using hydrogen gas to $\mathrm{H}_{2} \mathrm{~N}-\left(\mathrm{CH}_{2}\right)_{6}-\mathrm{NH}_{2}$, which is used in the production of nylon. What current must be used to produce $150 . \mathrm{kg}$ $\mathrm{NC}-\left(\mathrm{CH}_{2}\right)_{4}-\mathrm{CN}$ per hour?

One of the few industrial-scale processes that produce organic compounds electrochemically is used by the Monsanto Company to produce 1,4 -dicyanobutane. The reduction reaction is
$$2 \mathrm{CH}_{2}=\mathrm{CHCN}+2 \mathrm{H}^{+}+2 \mathrm{e}^{-} \longrightarrow \mathrm{NC}-\left(\mathrm{CH}_{2}\right)_{4}-\mathrm{CN}$$
The $\mathrm{NC}-\left(\mathrm{CH}_{2}\right)_{4}-\mathrm{CN}$ is then chemically reduced using hydrogen gas to $\mathrm{H}_{2} \mathrm{~N}-\left(\mathrm{CH}_{2}\right)_{6}-\mathrm{NH}_{2}$, which is used in the production of nylon. What current must be used to produce $150 . \mathrm{kg}$ $\mathrm{NC}-\left(\mathrm{CH}_{2}\right)_{4}-\mathrm{CN}$ per hour?

Key Concepts

Faraday's Law of Electrolysis

Faraday's Law of Electrolysis is a fundamental principle that relates the amount of substance transformed at an electrode during an electrochemical reaction to the total electric charge passed through the system. This principle uses Faraday's constant (approximately 96485 coulombs per mole of electrons) to connect the moles of electrons transferred and the production rate, making it essential for calculating the current needed in an electrochemical process.

Electrochemical Reaction Stoichiometry

The stoichiometry of an electrochemical reaction determines the ratio of electrons required to convert reactants into products. By analyzing the balanced chemical equation, one can discern the number of electrons that need to be transferred per mole of product formed. This concept is critical for linking the mass of a compound produced with the total charge required in the reaction.

Current-Charge-Time Relationship

The relationship between current, charge, and time is governed by the equation Q = I × t, where Q is the total charge in coulombs, I is the current in amperes, and t is the time in seconds. This relationship allows for the conversion of the calculated total charge into a necessary current over a specific time period, such as per hour, making it vital for designing industrial-scale electrochemical processes.

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