Question

On carrying out the electrolysis of acidified water, the volume of hydrogen liberated at $STP$ condition is $22.4L$. The volume of oxygen liberated is:

• A. $22.4L$
• B. $44.8L$
• C. $11.2L$
• D. $2.24L$

Answer 1

Answer: (C)

$11.2L$

The balanced chemical equation for the electrolysis of water is
$2H_{2}O\to 2H_2+O_2$
Thus, the ratio of the volume of hyrogen produced to the volume of oxygen produced is $2:1$
Thus, when $22.4$ L hydrogen is liberated, $11.2$ L oxygen is liberated.