How many liters of oxygen will it take to burn 1.12 liters of carbon monoxide (2)?

V = 1.12L; Chl-?

2CO + O2 = 2CO2 + Q – combustion, carbon monoxide is released (4);
Based on the proportions, we determine the amount of starting substances:
1 mol of gas at normal level – 22.4 l

X mol (CO) -1.12 L hence, X mol (CO) = 1 * 1.12 / 22.4 = 0.05 mol.

0.05 mol (CO) – X mol (O2);

-2 mol -1 mol from here, X mol (O2) = 0.05 * 1/2 = 0.025 mol.

We find the volume of O2:
V (O2) = 0.025 * 22.4 = 0.56 L

Answer: to burn carbon monoxide (2), you need oxygen with a volume of 0.56 liters