Electrolysis of dilute aqueous NaCl solution was carried out by passing 10 milli ampere current. The time required to liberate \(0.01 \mathrm{~mol}\) of \(\mathrm{H}_{2}\) gas at the cathode is (1 Faraday \(=96500 \mathrm{C} \mathrm{mol}^{-1}\) ) (A) \(9.65 \times 10^{4} \mathrm{sec}\) (B) \(19.3 \times 10^{4} \mathrm{sec}\) (C) \(28.95 \times 10^{4} \mathrm{sec}\) (D) \(38.6 \times 10^{4} \mathrm{sec}\)

Electrolysis is a chemical process that uses electrical current to drive a non-spontaneous reaction. It's typically conducted in an electrolytic cell where an electrolyte, such as aqueous sodium chloride (NaCl), is decomposed into its constituent elements. The key components in an electrolysis setup are the anode (positive electrode) and cathode (negative electrode).

When current is passed through the cell, chemical reactions occur at the electrodes, resulting in the liberation of substances like gases or the deposition of metals. For example, electrolysis of aqueous NaCl solution produces chlorine gas at the anode and hydrogen gas at the cathode. Understanding the concept of electrolysis is crucial in various applications, including electroplating, purification of metals, and the large-scale production of substances like chlorine and hydrogen.

The molar gas volume is the volume occupied by one mole of a gas at specified conditions of temperature and pressure. At standard temperature and pressure (STP - 0°C and 1 atm), one mole of any gas occupies approximately 22.4 liters. This concept is vital for understanding gas-related experiments, including those that involve electrolysis.

The volume of gas liberated during electrolysis can be calculated using the amount (in moles) of the gas produced. If we take the experiment given in our original exercise, it’s stated that 0.01 mole of hydrogen gas is produced. If you were to calculate the volume that this quantity of hydrogen would occupy at STP, it would be a straightforward application of the molar gas volume concept.

Stoichiometry is the section of chemistry that deals with the relationships between the quantities of reactants and products in a chemical reaction. It is the quantitative aspect that involves the use of mole concept and molar ratios as seen in balanced chemical equations.

In the context of Faraday's law of electrolysis, stoichiometry comes into play when we determine the number of moles of electrons required to produce a certain amount of gas. This assessment revolves around a balanced half-reaction equation for the generation of hydrogen gas: \(2H^+ + 2e^- \rightarrow H_2\). Here, stoichiometry tells us that 2 moles of electrons are needed to produce 1 mole of hydrogen gas. In our exercise, for 0.01 mole of \(H_2\), we need twice as many moles of electrons, which is an application of stoichiometry in calculating the total charge needed for electrolysis.

Chemical reactions are processes in which substances, the reactants, are transformed into different substances, the products. These reactions can vary greatly in their properties, such as reaction rates, enthalpy changes (exothermic or endothermic), and the states of matter involved.

In the case of the electrolysis problem we’re discussing, the chemical reaction is the decomposition of water (a component of the aqueous NaCl solution) to form hydrogen gas at the cathode through a reduction reaction. Understanding the types of chemical reactions involved in electrolysis is essential because it informs us which products will be formed at each electrode, the stoichiometry of the reaction, and hence the amount of electrical charge needed to produce a desired amount of substance through electrolysis.