What volume of carbon monoxide is required to react with 32.5 liters of oxygen gas according to the following reaction? (All gases are at the same temperature and pressure.)

carbon monoxide (g) + oxygen (g) carbon dioxide (g)

65 L is the volume of CO required

Explanation:

This is the reaction:

2CO (g) + O₂ (g) → 2CO₂ (g)

We must work with density to solve this problem

Density = Mass / volume

Let's determine the moles of O₂

1.43 g/mL = mass / 32500 mL

Notice, that we had to convert the volume from L, to mL, because the units of density.

Mass of O₂ → 1.43 g/mL. 32500 mL = 46475 g

Let's convert the mass to moles (mass / molar mas)

46475 g / 32 g/mol = 1452.3 moles

So ratio is 1:2

1 mol of oxygen needs 2 moles of CO, to react

Then, 1452.3 moles of O₂ would need the double of CO to react

1452.3 moles. 2 = 2904.6 moles of CO

This moles are contained in (mol. molar mass) =

2904.6 mol. 28 g/mol = 81328.8 g

Density of CO = Mass of CO / Volume of CO

1.25 g/mL = 81328.8 g / Volume of CO

81328.8 g / 1.25 g/mL = 65063 mL

If we convert to L

65063 mL = 65.0 L