A quantity of electric charge brings about the deposition of 3.28 g Cu at a cathode during the e

step 1 my name is Ahmad Ali in this simple question when he said that the charge of the copper is equal

A quantity of electric charge brings about the deposition of...

A quantity of electric charge brings about the deposition of $3.28 \mathrm{g}$ Cu at a cathode during the electrolysis of a solution containing $\mathrm{Cu}^{2+}(\text { aq })$. What volume of $\mathrm{H}_{2}(\mathrm{g}),$ measured at $28.2^{\circ} \mathrm{C}$ and $763 \mathrm{mm} \mathrm{Hg},$ would be produced by this same quantity of electric charge in the reduction of $\mathrm{H}^{+}($ aq) at a cathode?

A quantity of electric charge brings about the deposition of $3.28 \mathrm{g}$ Cu at a cathode during the electrolysis of a solution containing $\mathrm{Cu}^{2+}(\text { aq })$. What volume of $\mathrm{H}_{2}(\mathrm{g}),$ measured at $28.2^{\circ} \mathrm{C}$ and $763 \mathrm{mm} \mathrm{Hg},$ would be
produced by this same quantity of electric charge in the reduction of $\mathrm{H}^{+}($ aq) at a cathode?

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Key Concepts

Ideal Gas Law

The Ideal Gas Law is a fundamental equation used to relate the pressure, volume, temperature, and number of moles of a gas. In the context of electrolysis, it is applied to calculate the volume of gas generated from a known amount of moles produced during the reaction, under specified temperature and pressure conditions.

Faraday's Laws of Electrolysis

These laws establish the quantitative relationship between the amount of electrical charge passed through an electrolyte and the amount of substance that is deposited or liberated at the electrodes. They allow one to calculate the number of moles of reactant transformed by knowing the total charge and using the Faraday constant, which relates the charge carried per mole of electrons.

Electrolysis Stoichiometry

This concept involves understanding the stoichiometric relationships between the electrons transferred in a half-reaction and the substances being reduced or oxidized. It is used to determine how many moles of electrons are required to achieve a given chemical change, such as depositing a metal or forming a gas, and then linking that to the quantity produced in another half-reaction.

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