Question

Describe the reactions during the electrolysis of water in an electrolytic cell. Describe the reactions during the electrolysis of water in an electrolytic cell. Oxygen and hydrogen are both reduced. Oxygen is oxidized and hydrogen is reduced. Neither oxygen or hydrogen are oxidized or reduced. Oxygen and hydrogen are both oxidized. Oxygen is reduced and hydrogen is oxidized.

Answer 1

During the electrolysis of water, oxygen is oxidized at the anode to produce oxygen gas and hydrogen ions, while hydrogen is reduced at the cathode to generate hydrogen gas and hydroxide ions.

Step-by-step explanation:

Description of the Electrolysis of Water

During the electrolysis of water, hydrogen and oxygen gases are produced. Oxygen is produced at the anode through the oxidation of water molecules resulting in the formation of oxygen gas and hydrogen ions (H+). Simultaneously, at the cathode, water molecules are reduced to produce hydrogen gas and hydroxide ions (OH-). As these reactions occur, electrons are transferred, reflecting the characteristics of a redox reaction.

To elaborate on the reactions at each electrode: at the anode, oxidation occurs with water molecules losing electrons to form oxygen gas, which can be represented as 2H2O –> O2 + 4H+ + 4e−, and at the cathode, reduction happens where hydrogen ions gain electrons to form hydrogen gas, represented by the half-reaction: 2H+ + 2e− –> H2.

It is important to correct the initial statement where it was mentioned both oxygen and hydrogen are either oxidized or reduced; in fact, oxygen is oxidized and hydrogen is reduced. A conductive electrolyte such as H2SO4 is usually added to the water to enhance the process by increasing the availability of ions which facilitate the flow of electrons.

Answer 2

Oxygen is oxidized and hydrogen is reduced

Step-by-step explanation:

In the electrolysis of water, a pair of Platinum electrodes are immersed in water. Th water has a small quantity of either an acid, salt or base, in most cases H2S04, added to it, to aid ionization. This is because water on its own does not posses enough ions to undergo electrolysis. At the platinum anode, water is oxidized to oxygen gas and hydrogen ions. At the platinum cathode, water is reduced to hydrogen gas and hydroxide ions. The proportion of oxygen and hydrogen produced should be theoretically 1 : 2 respectively, but is not usually so, due to competing side reactions. The hydrogen by product is usually used as a fuel source, and it usually combine with the hydroxide ion to form water back again.