Question

The combustion of gasoline produces carbon dioxide and water. assume gasoline to be pure octane (c8h18) and calculate the mass (in kg) of carbon dioxide that is added to the atmosphere per 1.7 kg of octane burned. (hint: begin by writing a balanced equation for the combustion reaction.)

Answer 1

the balanced equation for combustion of octane is given below
2C₈H₁₈ + 25O₂  ---> 16CO₂ + 18H₂O
stoichiometry of octane to carbon dioxide is 2:16
number of moles of octane burnt - 1700 g / 114.2 g/mol = 14.88 mol
For every 2 mol of octane - 16 mol of CO₂ is formed 
Therefore for 14.88 mol of octane - 16/2 x 14.88 mol = 119.0 mol of CO₂
Mass of CO₂ formed - 119.0 mol x 44 g/mol = 5236 g
mass of CO₂ formed - 5.236 kg

Answer 2

The mass of carbon dioxide that is added to the atmosphere per 1.7 kg of octane burned is 5.236 kg

What is a combustion reaction?

A combustion reaction is one in which the substance reacts with oxygen to produce heat and light.

The combustion reaction is

2C₈H₁₈ + 25O₂  = 16CO₂ + 18H₂O

By stoichiometry

octane : carbon dioxide

         2: 16

Calculating the number of moles

$\rm Number\;of \;moles= \dfrac{mass}{molar\;mass}\\\\\rm Number\;of \;moles= \dfrac{1700 g }{114.2 g/mol}= 14.48\;mol$

Now, according to stoichiometry,

The 14.48 moles of octane will be

$\dfrac{6}{2}\times 14.88 mol = 119.0\; mol\; of\; CO_2$

Mass of carbon dioxide will be

119.0 mol × 44 g/mol = 5236 g

Thus, the mass of carbon dioxide is 5.236 kg

Learn more about combustion, here:
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