In the electrolysis of a sodium chloride solution, what volume of H2(g) is produced in the same

step 1 This is an interesting question. We can use the ideal gas law to calculate the moles of CL2 that

In the electrolysis of a sodium chloride solution, what...

In the electrolysis of a sodium chloride solution, what volume of $\mathrm{H}_{2}(g)$ is produced in the same time it takes to produce $257 \mathrm{~L}$ $\mathrm{Cl}_{2}(\mathrm{~g})$, with both volumes measured at $50 .{ }^{\circ} \mathrm{C}$ and $2.50 \mathrm{~atm} ?$

Key Concepts

Ideal Gas Law

The ideal gas law, expressed as PV = nRT, connects the pressure, volume, temperature, and amount (in moles) of a gas. In the context of electrolysis where gases are produced, this law allows us to convert between the volume of a gas and the number of moles, as long as the pressure and temperature are known. This is crucial when comparing gas volumes measured under the same conditions to infer the underlying stoichiometric relationships.

Electrolysis

Electrolysis is a process that uses an electric current to drive a non-spontaneous chemical reaction. It involves the transfer of electrons that results in the decomposition of compounds into their constituent elements or simpler compounds. This concept is fundamental in understanding how substances like sodium chloride in solution can be split into gaseous products.

Chemical Stoichiometry and Reaction Balancing

Chemical stoichiometry involves using a balanced chemical equation to determine the relative amounts of reactants and products in a reaction. In processes like the electrolysis of sodium chloride solution, a balanced reaction reveals the mole-to-mole ratios between different gaseous products such as chlorine and hydrogen. This ratio is essential for predicting how much of one product is formed when the other is obtained in a certain amount.

Faraday's Laws of Electrolysis

Faraday's laws of electrolysis relate the quantity of electric charge passed through an electrolytic cell to the amount of substance produced at the electrodes. This concept supports the stoichiometric analysis by showing that, under constant current, the amounts of products formed are directly proportional to the number of electrons exchanged during the chemical reaction.

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