Answer:

The ratio of hydrogen to oxygen formed at the cathode and anode during electrolysis of water is 2:1 by volume because water (H₂O) molecules are split into hydrogen and oxygen gases in a 2:1 ratio through the electrolysis process, where two moles of hydrogen gas are produced for every one mole of oxygen gas, and gases occupy volumes in simple whole number ratios.

Explanation:

The given statement refers to the electrolysis of water. In the electrolysis of water, water molecules (H₂O) are split into hydrogen (H₂) and oxygen (O₂) gases through the process of electrolysis, which occurs in the presence of an electric current.

At the cathode (negative electrode), hydrogen gas (H₂) is produced through the reduction reaction:

2

�

2

�

(

�

)

+

2

�

−

→

2

�

�

−

(

�

�

)

+

�

2

(

�

)

2H

2

​

O(l)+2e

−

→2OH

−

(aq)+H

2

​

(g)

At the anode (positive electrode), oxygen gas (O₂) is produced through the oxidation reaction:

4

�

2

�

(

�

)

→

4

�

−

+

�

2

(

�

)

+

4

�

+

(

�

�

)

4H

2

​

O(l)→4e

−

+O

2

​

(g)+4H

+

(aq)

The ratio of hydrogen to oxygen production at the cathode and anode is 2:1 by volume. This ratio is based on the stoichiometry of the chemical reactions involved in the electrolysis of water. For every two moles of hydrogen gas produced, one mole of oxygen gas is produced. Since gases occupy volumes in simple whole number ratios, the volume ratio is also 2:1 for hydrogen to oxygen.

Answer:

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