5.6 g of carbon monoxide is heated with excess of O2 to form carbon dioxide. What is the theoretical yield in grams of carbon dioxide (2CO + O2 ---> 2CO2)?

Explanation

The balanced equation is: 2CO + O2 → 2CO2 From the balanced equation, we can see that the molar ratio between CO and CO2 is 2:2, meaning that 2 moles of CO react to form 2 moles of CO2. First, let's determine the number of moles of CO: Molar mass of CO = 12.01 g/mol (carbon) + 16.00 g/mol (oxygen) = 28.01 g/mol Moles of CO = mass of CO / molar mass of CO = 5.6 g / 28.01 g/mol ≈ 0.199 moles Since the molar ratio between CO and CO2 is 2:2, we can conclude that 0.199 moles of CO will produce an equal number of moles of CO2. Therefore, the theoretical yield of CO2 is also 0.199 moles. Now, let's calculate the mass of CO2: Molar mass of CO2 = 12.01 g/mol (carbon) + 16.00 g/mol (oxygen) + 16.00 g/mol (oxygen) = 44.01 g/mol Mass of CO2 = moles of CO2 * molar mass of CO2 = 0.199 moles * 44.01 g/mol ≈ 8.8 g