If you have 2.63 grams of the organic fuel (MW=74.09 g / mol) and 5.63 grams of oxygen gas, how many grams of carbon dioxide will you produce?

Mass of CO₂ = 3.08 g

Explanation:

Given dа ta:

Mass of organic fuel = 2.63 g

Molar mass of organic fuel = 74.09 g/mol

Mass of oxygen = 5.63 g

Mass of carbon dioxide = ?

Solution:

Chemical equation:

2C₃H₆O₂ + 7O₂ → 6CO₂ + 6H₂O

Number of moles of organic fuel:

Number of moles = mass / molar mass

Number of moles = 2.63 g / 74.09 g/mol

Number of moles = 0.035 mol

Number of moles of oxygen:

Number of moles = mass / molar mass

Number of moles = 5.63 g / 32 g/mol

Number of moles = 0.176 mol

Now we will compare the moles of O₂ and C₃H₆O₂ with CO.

C₃H₆O₂ : CO

3 : 6

0.035 : 6/3 * 0.035 = 0.07

O₂ : CO

7 : 6

0.176 : 6/7 * 0.176 = 0.151 mol

The number of moles of CO₂ produced by C₃H₆O₂ are less it will be limiting reactant.

Mass of carbondioxide:

Mass of CO₂ = moles * molar mass

Mass of CO₂ = 0.07 mol * 44 g/mol

Mass of CO₂ = 3.08 g