When the amount of oxygen is limited, carbon and oxygen react to form carbon monoxide. How many grams of CO can be formed from 35.0 grams of oxygen? 2C + O2 → 2CO Using 32.00 g/mole as the molecular mass of oxygen and 28.01 g/mole as the molecular mass of carbon monoxide, solve the above problem.

The formula that denotes the incomplete combustion of carbon in the presence of a limited amount of oxygen is 2 C + O ₂ → 2 CO

If the mass of oxygen that is used to combust carbon is 35 g

then the moles of oxygen = mass of oxygen : molar mass of oxygen

= 35 g : 32 g/mol

= 1.0938 mol

Now, the mole ratio of oxygen : carbon monoxide based on the balance equation is 1 : 2

⇒ If the mole of oxygen = 1.0938 mol

then the mole of carbon monoxide = 1.0938 * 2

= 2.1876 mol

Mass of CO is = mol of CO * molar mass of CO

= 2.1876 mol * 28 g/mol

= 61.25 g

∴ when a certain mass of carbon is combusted in 35g of oxygen then it produces approx. 61.25 g of Carbon Monoxide.