Electrolysis of dilute \(\mathrm{H}_{2} \mathrm{SO}_{4}\) will give: (a) \(\mathrm{SO}_{2}\) and \(\mathrm{O}_{2}\) (b) \(\mathrm{H}_{2}\) and \(\mathrm{O}_{2}\) (c) \(\mathrm{H}_{2} \overline{\mathrm{O}}\) and \(\mathrm{H}_{2}\) (d) \(\mathrm{SO}_{2}\) and \(\mathrm{H}_{2}\)

Electrolysis is an intriguing process involving electrochemical cell reactions. In this process, electrical energy is used to drive a non-spontaneous chemical reaction. This is notably different from a battery, where naturally occurring chemical reactions produce electrical energy. With electrolysis, the setup consists of two electrodes, the cathode and the anode, submerged in an electrolytic solution - in our example, dilute sulfuric acid.

When an electric current is passed through the solution, the electrolyte's ions move towards the electrodes where they either gain or lose electrons. At the cathode, cations (positively charged ions) are reduced by gaining electrons, whereas, at the anode, anions (negatively charged ions) are oxidized by losing electrons. The specific reactions that occur depend on the nature of the electrolyte and the electrodes. For dilute sulfuric acid electrolysis, hydrogen ions are reduced to hydrogen gas at the cathode, and water molecules are oxidized to oxygen gas at the anode.

The concept of dissociation is central to understanding electrolysis. Dissociation is the process in which an ionic compound separates into its individual ion components in solution. With dilute sulfuric acid, \(\mathrm{H}_2\mathrm{SO}_4{}\), this dissociation is pivotal as it provides the ions necessary for the electrochemical reactions.

Upon adding sulfuric acid to water, it dissociates into hydrogen ions \(\mathrm{H}^+\) and sulfate ions \(\mathrm{SO}_4^{2-}\). This dissociation is vital for the upcoming reactions during electrolysis. Hydrogen ions, being charged, will migrate towards the cathode where they can then be reduced to form hydrogen gas. Notably, the availability of these ions is what makes the entire process possible, as they carry the electrical current through the solution.

Lastly, the heart of electrolysis lies in the oxidation and reduction reactions. These reactions are collectively known as redox reactions. In every redox reaction, one species loses electrons (oxidation), and another species gains electrons (reduction).

In the context of electrolyzing dilute sulfuric acid, at the cathode, the reduction reaction results in the formation of hydrogen gas from hydrogen ions, \(2\mathrm{H}^+ + 2e^- \rightarrow \mathrm{H}_2(g)\). Conversely, at the anode, the oxidation of water molecules yields oxygen gas, alongside hydrogen ions and electrons, \(2\mathrm{H}_2\mathrm{O}(l) \rightarrow 4\mathrm{H}^+ + 4e^- + \mathrm{O}_2(g)\).

Understanding these reactions is fundamental, as they determine the substances that are produced at each electrode. Redox reactions ensure that charge is conserved in the system, making electrolysis a balanced process in terms of electrons gained and lost.