Question

If the weight ratio of $C$ and $O_2$ present is 1:2 and both of reactants completely consume and form $CO$ and $C{O}_2$. We will obtain a gaseous mixture of $CO$ and $C{O}_2$ in the ratio:

• A. 11:7
• B. 7:11
• C. 1:1
• D. 1:2

Answer 1

Answer: (B)

7:11

$\underset{w}{C}+\underset{2w}{O_2}\to \underset{x}{CO}+\underset{y}{C{O}_2}$

By applying the concept of principle of Atom Conservation (POAC) to carbon $\frac{w}{12}=\frac{x}{28}+\frac{y}{44}$

$\frac{w}{3}=\frac{x}{7}+\frac{y}{11}$ ......(1)

By applying the concept of principle of atom conservation (POAC) to oxygen $2\times \frac{2w}{32}=\frac{x}{28}+2\times \frac{y}{44}$

$\frac{w}{4}=\frac{x}{14}+\frac{y}{11}$ ......(2)

Hence, $\frac{3y}{11}+\frac{3x}{7}=\frac{4x}{14}+\frac{4y}{11}$

$\frac{3x}{7}-\frac{2x}{7}=\frac{y}{11}$

$\frac{x}{7}=\frac{y}{11},\frac{x}{y}=7:11$. This is the ratio of $CO$ and $C{O}_2$ in the gaseous mixture.