Question

What volume of $C{O}_2$ will be liberated at STP (1 atm, 273 K), If $7.2$ gm of carbon is burnt in excess of oxygen?

• A. $11.2$ L
• B. $13.4$ L
• C. $2.24$ L
• D. $1.12$ L

Answer 1

The correct option is B $13.4$ L

$C$ + $O_2$ $\to$ $C{O}_2$
We have given $7.2$ gm of C and Volume of $C{O}_2$ at STP is asked.
Moles of Carbon = $\frac{7.2}{12}=0.6mol$
As per stoichiometry,
1 mol of $C$ produces 1 mol of $C{O}_2$.
Hence, $0.6$ mol of $C$ produces $0.6$ mol of $C{O}_2$

$\therefore V_{C{O}_2}=n_{C{O}_2}\times 22.4$
$\therefore V_{C{O}_2}=0.6\times 22.4=13.44L$