The mass of a gold atom is 3.27 ×10^-25 kg. If 1.25 kg of gold is deposited on the negative elec

step 1 Here gold ions are electrochemically reduced to gold metal and we have to calculate the current

The mass of a gold atom is 3.27 ×10^-25 kg. If 1.25 kg of...

The mass of a gold atom is $3.27 \times 10^{-25} \mathrm{kg}$. If $1.25 \mathrm{kg}$ of gold is deposited on the negative electrode of an electrolytic cell in a period of $2.78 \mathrm{h}$, what is the cur. rent in the cell in this period? Assume that each gold ion carries one elementary unit of positive charge.

Key Concepts

Electric Current

Electric current is defined as the rate at which charge flows through a conductor or a circuit. In electrolysis problems, determining the current involves calculating the total charge transferred and dividing by the time interval over which the reaction occurs, establishing a direct link between the chemical process and the electrical parameters in the system.

Elementary Charge

The elementary charge is the fundamental unit of electric charge carried by a single proton or the negative of that carried by a single electron. It is used to convert the number of charged particles (such as ions or electrons) into the total electric charge, which is essential for connecting microscopic events in the cell to macroscopic electrical measurements.

Electrolysis

Electrolysis involves driving a non-spontaneous chemical reaction using electrical energy. In an electrolytic cell, ions in a solution or molten state migrate to electrodes where reduction (gain of electrons) or oxidation (loss of electrons) occurs, resulting in the deposition or dissolution of substances. Understanding electrolysis is essential when analyzing processes where material is deposited on an electrode as a result of an applied current.

Faraday's Laws of Electrolysis

Faraday's laws relate the amount of substance deposited at an electrode to the total electric charge passed through the electrolyte. They state that the mass of the substance altered at an electrode during electrolysis is proportional to the quantity of electricity used, linking the physics of current and time with the chemistry of mass change.

Atomic and Molar Conversions

This concept involves converting between mass, number of atoms, and moles using the atomic mass of a substance. It is crucial for determining the total number of atoms involved in a reaction, as calculations often require converting the given mass into moles and then into individual atoms when relating chemical changes to electrical charge.

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