A major component of gasoline is octane (C8H18). When liquid octane is burned in air it reacts with oxygen (O2) gas to produce carbon dioxide gas and water vapor. Calculate the moles of carbon dioxide produced by the reaction of 2.00 mol of oxygen. Be sure your answer has a unit symbol, if necessary, and round it to 3 significant digits.

The balanced chemical equation for the combustion of octane (C₈H₁₈) in air is:

\[
2 \, \text{C}_8\text{H}_{18} + 25 \, \text{O}_2 \rightarrow 16 \, \text{CO}_2 + 18 \, \text{H}_2\text{O}
\]

This equation tells us that for every 25 moles of oxygen (\( \text{O}_2 \)), 16 moles of carbon dioxide (\( \text{CO}_2 \)) are produced.

Now, we can set up a proportion to find out how many moles of carbon dioxide are produced when 2.00 moles of oxygen are reacted:

\[
\frac{16 \, \text{mol} \, \text{CO}_2}{25 \, \text{mol} \, \text{O}_2} = \frac{x \, \text{mol} \, \text{CO}_2}{2.00 \, \text{mol} \, \text{O}_2}
\]

Solving for \( x \), which represents the moles of \( \text{CO}_2 \):

\[
x = \frac{16}{25} \times 2.00 = 1.28 \, \text{mol} \, \text{CO}_2
\]

Thus, the moles of carbon dioxide produced is:

\[
1.28 \, \text{mol} \, \text{CO}_2
\]

Let me know if you want more details or have questions! Here are some related questions to consider:

1. What is the molar mass of octane (C₈H₁₈)?
2. How many moles of water vapor are produced in this reaction?
3. What volume of carbon dioxide gas is produced at standard temperature and pressure (STP)?
4. How many grams of oxygen are required for the combustion of 1 mole of octane?
5. What is the total number of molecules of carbon dioxide produced in this reaction?

**Tip:** When dealing with combustion reactions, it's helpful to memorize the basic reaction format for hydrocarbons: hydrocarbon + oxygen → carbon dioxide + water.

Calculate the moles of carbon dioxide produced when burning 2.00 moles of oxygen during the combustion of octane (C8H18). This problem demonstrates key concepts in stoichiometry and chemical reactions, suitable for high school students studying chemistry.

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