Chemistry Question from JEE Main 2023 · 31 January, Shift 2

Assume carbon burns according to the following equation: $2C(s) + O_2(g) \rightarrow 2CO(g)$ When $12 \, \text{g}$ of carbon is burnt in $48 \, \text{g}$ of oxygen, the volume of carbon monoxide produced is $\_ \times 10^{-1}$ L at STP (nearest integer).

Given: Assume CO as ideal gas, Mass of C is $12 \, \text{g mol}^{-1}$, Mass of O is $16 \, \text{g mol}^{-1}$, and molar volume of an ideal gas at STP is $22.7 \, \text{L mol}^{-1}$.