Question

The volume of oxygen at $STP$ required to burn $2.4g$ of carbon completely is:

• A. $1.12L$
• B. $8.96L$
• C. $2.24L$
• D. $4.48L$

Answer 1

The correct option is D $4.48L$

The chemical equation for the process is:

$C+O_2\to C{O}_2$

For the above reaction, 1 mole of $O_2$ will burn 1 mole of $C$ completely.

In $2.4g$ C, number of moles =$\frac{2.4}{12}=0.2$ moles of oxygen is required.

Volume occupied by 1 mole of an ideal gas at STP ($T=0K$ and $P=1atm$) is $22.4L$.

Therefore, 0.2 mol $O_2=0.2\times 22.4L$

$=4.48L$.

Option $D$ is the correct answer.