The apparatus in Figure P 17.7 is used for the electrolysis of water. Hydrogen and oxygen gas ar

step 1 The figure, the figure 17 -7 shows an apparatus for the electrolysis of water. Hydrogen is being

The apparatus in Figure P 17.7 is used for the electrolysis...

The apparatus in Figure $\mathrm{P} 17.7$ is used for the electrolysis of water. Hydrogen and oxygen gas are collected in the two inverted burets. An inert electrode at the bottom of the left buret is connected to the negative terminal of a 6 -volt battery; the electrode in the buret on the right is connected to the positive terminal. A small quantity of sulfuric acid is added to speed up the electrolytic reaction. a. What are the half-reactions at the left and right electrodes and their standard potentials? b. Why does sulfuric acid make the electrolysis reaction go more rapidly? (FIGURE CANNOT COPY)

The apparatus in Figure $\mathrm{P} 17.7$ is used for the electrolysis of water. Hydrogen and oxygen gas are collected in the two inverted burets. An inert electrode at the bottom of the left buret is connected to the negative terminal of a 6 -volt battery; the electrode in the buret on the right is connected to the positive terminal. A small quantity of sulfuric acid is added to speed up the electrolytic reaction.
a. What are the half-reactions at the left and right electrodes and their standard potentials?
b. Why does sulfuric acid make the electrolysis reaction go more rapidly?
(FIGURE CANNOT COPY)

Key Concepts

Electrolysis

Electrolysis is a process that uses direct electrical current to drive a non-spontaneous chemical reaction. In the context of water splitting, electrolysis involves breaking water molecules into hydrogen and oxygen gases. This process typically requires an electrolyte to improve conductivity between electrodes, facilitating the movement of ions that carry charge through the solution.

Half-Reactions

Half-reactions are individual oxidation or reduction reactions that occur at each electrode during electrolysis. At the cathode (negative electrode), reduction takes place whereby water molecules gain electrons to form hydrogen gas. Conversely, at the anode (positive electrode), oxidation occurs, and water molecules lose electrons to produce oxygen gas. These separated reactions combine to yield the overall decomposition of water.

Standard Electrode Potentials

Standard electrode potentials refer to the inherent tendency of a chemical species to be reduced or oxidized under standard conditions. Each half-reaction in an electrochemical process is associated with a standard potential, which helps predict the direction of electron flow and the feasibility of the reaction. In water electrolysis, the standard reduction potential for the hydrogen evolution (cathode) and the standard oxidation potential for the oxygen evolution (anode) provide insight into the energy requirements of the process.

Role of Electrolytes in Electrolysis

The addition of an electrolyte, such as sulfuric acid, increases the conductivity of the water by providing more ions in solution. This enhanced ion presence lowers the solution's resistance, allowing the electric current to pass more easily through the medium. As a result, the electrolysis reaction proceeds more rapidly because the charge transfer at the electrodes is facilitated, improving the overall efficiency of the water-splitting process.

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