Question

The reaction of burning of carbon in oxygen is represented by equation:
$C_{\left(s\right)}+O_{2\left(g\right)}⟶{CO}_{2\left(g\right)}+$ Heat $+$ Light

When $9.0g$ of solid carbon is burnt in $16.0g$ of oxygen gas, $22.0g$ of carbon dioxide gas formed on burning of $3.0g$ of carbon in $32.0g$ of oxygen would be: (Note : atomic mass of $C=12.0u,O=16.0u$)

• A. $16.60g$
• B. $7.33g$
• C. $8.25g$
• D. $11.00g$

Answer 1

Answer: (D)

$11.00g$

Given,

• Weight of carbon $=3g$.

Atomic mass of carbon $=12g$.
$\therefore$ Moles of carbon = $\frac{1}{4}$.

• Weight of oxygen$=32g$.

Atomic mass of oxygen$=16g$.
$\therefore$ Moles of oxygen = $\frac{32}{32}$ = 1

• Now out of 1 mole of oxygen, $\frac{1}{4}$ mole will react with $\frac{1}{4}$ mole of carbon.

$\therefore MassofC{O}_2=3+\frac{1}{4}\times 32=11g$.