Question

What is the ratio of hydrogen to oxygen by volume after decomposing the water by an electric current?
A. $1:8$
B. $1:2$
C. $1:9$
D. $2:1$

Answer 1

Hint: We have to know that electrolysis is characterized as a cycle of deteriorating ionic mixtures into their components by passing an immediate electric flow through the compound in a liquid structure. The cations are decreased at cathode and anions are oxidized at the anode.

Complete answer:
We have to know that electrolysis is passing an electric flow through a fluid containing particles with the goal that decay response happens.
At the point when an electric flow is gone through fermented water, it breaks down to give hydrogen and oxygen gas. The hydrogen gas is obtained at the cathode and the oxygen gas is acquired at the anode.
The response for deterioration of water into oxygen and hydrogen is as per the following:
$2{H_2}O \to 2{H_2} + {O_2}$
Accordingly, the quantity of hydrogen particles delivered is double the quantity of oxygen atoms. Along these lines, electrolysis of water produces two volumes of hydrogen gas and one volume of oxygen gas on the grounds that the proportion of hydrogen and oxygen components in water is $2:1$ by volume. Consequently, the measure of gases gathered in two test tubes isn't equivalent.
Therefore, the ratio of hydrogen to oxygen by volume after decomposing the water by an electric current is $2:1$ .

So, the correct answer is “Option D”.

Note:
During electrolysis, decidedly charged particles move to the negative anode and adversely charged particles move to the positive cathode. Then, at that point emphatically charged particles get electrons and contrarily charged particles lose electrons. Both the results of the separation get gathered at the anodes.