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The problem you're working with involves the combustion of hexane \((\text{C}_6\text{H}_{14})\) with oxygen \((\text{O}_2)\) to produce carbon dioxide \((\text{CO}_2)\) and water \((\text{H}_2\text{O})\). Here’s a step-by-step approach to calculate the percent yield of carbon dioxide, based on the data provided:

### Reaction:
The balanced equation for the combustion of hexane is:

\[
2\text{C}_6\text{H}_{14} + 19\text{O}_2 \rightarrow 12\text{CO}_2 + 14\text{H}_2\text{O}
\]

### Step 1: Molar Masses
- Molar mass of hexane \((\text{C}_6\text{H}_{14})\):
  \[
  (6 \times 12.01 \, \text{g/mol}) + (14 \times 1.008 \, \text{g/mol}) = 86.18 \, \text{g/mol}
  \]
- Molar mass of carbon dioxide \((\text{CO}_2)\):
  \[
  (1 \times 12.01 \, \text{g/mol}) + (2 \times 16.00 \, \text{g/mol}) = 44.01 \, \text{g/mol}
  \]

### Step 2: Find the Limiting Reactant
- Given: 
  - Mass of hexane: \(6.0 \, \text{g}\)
  - Mass of oxygen: \(9.4 \, \text{g}\)

#### Moles of hexane:
\[
\frac{6.0 \, \text{g}}{86.18 \, \text{g/mol}} = 0.0696 \, \text{mol}
\]

#### Moles of oxygen:
\[
\frac{9.4 \, \text{g}}{32.00 \, \text{g/mol}} = 0.29375 \, \text{mol}
\]

From the balanced equation, 2 moles of hexane require 19 moles of oxygen. Therefore, for 0.0696 moles of hexane:
\[
\text{Required oxygen} = 0.0696 \times \frac{19}{2} = 0.6612 \, \text{mol}
\]
Since we only have 0.29375 moles of oxygen, oxygen is the limiting reactant.

### Step 3: Theoretical Yield of Carbon Dioxide
From the balanced equation, 19 moles of oxygen produce 12 moles of carbon dioxide. Therefore, for 0.29375 moles of oxygen:
\[
\text{Moles of CO}_2 = 0.29375 \times \frac{12}{19} = 0.1855 \, \text{mol}
\]
Mass of carbon dioxide:
\[
\text{Mass of CO}_2 = 0.1855 \times 44.01 \, \text{g/mol} = 8.16 \, \text{g}
\]

### Step 4: Percent Yield
Given the actual mass of carbon dioxide produced is 5.72 g, the percent yield is calculated as:
\[
\text{Percent yield} = \frac{5.72 \, \text{g}}{8.16 \, \text{g}} \times 100 = 70.1\%
\]

### Final Answer:
The percent yield of carbon dioxide is **70.1%**.

Would you like more details on any part of the solution? 

Here are five related questions you might consider:
1. How would you calculate the percent yield if hexane were the limiting reactant?
2. What would happen to the percent yield if more oxygen were added to the reaction?
3. How does balancing chemical equations affect stoichiometric calculations?
4. Why is oxygen the limiting reactant in this scenario?
5. What are the practical implications of percent yield in industrial chemical reactions?

**Tip:** Always identify the limiting reactant first, as it dictates the theoretical yield in stoichiometry problems.

Liquid hexane (CH3(CH2)4CH3) reacts with gaseous oxygen gas (O2) to produce gaseous carbon dioxide (CO2) and gaseous water (H2O). If 5.72 g of carbon dioxide is produced from the reaction of 6.0 g of hexane and 9.4 g of oxygen gas, calculate the percent yield of carbon dioxide.

Learn how to calculate the percent yield of carbon dioxide produced in the combustion of hexane (C6H14) with oxygen (O2). This step-by-step solution includes key stoichiometric calculations, identification of the limiting reactant, and percent yield formula application.

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