JEE Main 2024 — Some Basic Concepts Of Chemistry Question with Solution

To find the number of moles of methane ($C{H}_4$) required to produce 11g of $C{O}_2$ upon complete combustion, we first need the balanced chemical equation for the combustion of methane:

$$C{H}_4+2O_2\to C{O}_2+2H_{2}O$$

From the balanced equation, we see that 1 mole of $C{H}_4$ produces 1 mole of $C{O}_2$. Therefore, the moles of $C{H}_4$ needed to produce a certain amount of $C{O}_2$ will be equal to the moles of $C{O}_2$ produced.

To find the moles of $C{O}_2$ produced from 11g of $C{O}_2$, we use the formula:

$$\text{Moles}=\frac{\text{Mass}}{\text{Molar mass}}$$

The molar mass of $C{O}_2$ is $44g/mol$ (12 from carbon and 16$\times$2 from oxygen). Then, the moles of $C{O}_2$ produced from 11g of $C{O}_2$ can be calculated as:

$$\text{Moles of }C{O}_2=\frac{11\mathrm{g}}{44g/mol}=0.25\mathrm{mol}$$

Since the stoichiometry of the reaction between methane and oxygen is 1:1 for $C{H}_4$ and $C{O}_2$, the moles of $C{H}_4$ required to produce 11g of $C{O}_2$ is also 0.25 moles.

Therefore, the correct answer is Option B: 0.25.