Describe the reactions during the electrolysis of water :

A) Oxygen is reduced and hydrogen is oxidized.

B) Oxygen and hydrogen are both oxidized.

C) Oxygen and hydrogen are both reduced.

D) Oxygen is oxidized and hydrogen is reduced.

E) Neither oxygen or hydrogen are oxidized or reduced.

Please give a reason why you chose that answer.

The hydrogen atom in the water molecule has been reduced since its oxidation snumber goes from 1⁺ to 0, and the oxygen has oxidized from 2⁻ to 0 , and in the balanced equation. The overall exchange of electron is 4.

sholadaniel1 sholadaniel1 · Answer 2 · 2019-12-03T14:03:54+01:00

Answer: D

Explanation:

Electrolysis of water which is also called water splitting, is the decomposition of water into oxygen and hydrogen gas when an electric current is passed through it, from a platinum electrode.

Pure water (H2O) is used to produce hydrogen gas (H2), which is fuel, and breathable oxygen gas(O2).

Hydrogen is collected at cathode and oxygen is collected at anode.

Chemical reaction

2 H2O(l) → 2 H2(g) + O2(g)

In the reactant H20, the oxidation state of Hydrogen is (+1) the oxidation state of Oxygen is (-2)

In the products, the oxidation number of elements in the uncombine state is zero so, the oxidation state of Hydrogen is 0 and Oxygen is 0.

Therefore Hydrogen is reduced (from +1 to 0)and oxygen is oxidized (from -2 to 0)

The half reaction are:

Reduction: 2 H+(aq) + 2e− → H2(g)

Oxidation: 2 H2O(l) → O2(g) + 4 H+(aq) + 4e−