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 data:

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

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