Assume carbon burns according to following equation : $2 \mathrm{C}_{(\mathrm{s})}+\mathrm{O}_{2(\mathrm{~g})} \rightarrow 2 \mathrm{CO}(\mathrm{g})$ When 12 g carbon is burnt in 48 g of oxygen, the volume of carbon monoxide produced is ___ × l0–1 L at STP [nearest integer] [Given : Assume CO as ideal gas, Mass of C is 12 g $\mathrm{mol}^{-1}$, Mass of O is 16 g $\mathrm{mol}^{-1}$ and molar volume of an ideal gas at STP is 22.7 $\mathrm{L} \mathrm{mol}^{-1}$]