Questions: On a separate sheet of paper, write out the problem using all the steps. Round using significant figures. How many moles of water are produced when 7.60 moles of propane (C3H8) combust in the presence of oxygen? C3H8 + O2 → CO2 + H2O

On a separate sheet of paper, write out the problem using all the steps. Round using significant figures. How many moles of water are produced when 7.60 moles of propane (C3H8) combust in the presence of oxygen? C3H8 + O2 → CO2 + H2O
Transcript text: 6) On a separate sheet of paper, write out the problem using all the steps. Round using significant figures. How many moles of water are produced when 7.60 moles of propane $\left(\mathrm{C}_{3} \mathrm{H}_{8}\right)$ combust in the presence of oxygen? \[ \mathrm{C}_{3} \mathrm{H}_{8}+\mathrm{O}_{2} \rightarrow \mathrm{CO}_{2}+\mathrm{H}_{2} \mathrm{O} \] Attach a file
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Solution

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Solution Steps

Step 1: Write the Balanced Chemical Equation

First, we need to write and balance the chemical equation for the combustion of propane (\(\mathrm{C}_{3} \mathrm{H}_{8}\)).

\[ \mathrm{C}_{3} \mathrm{H}_{8} + 5\mathrm{O}_{2} \rightarrow 3\mathrm{CO}_{2} + 4\mathrm{H}_{2} \mathrm{O} \]

Step 2: Identify the Mole Ratio

From the balanced equation, we can see the mole ratio between propane (\(\mathrm{C}_{3} \mathrm{H}_{8}\)) and water (\(\mathrm{H}_{2} \mathrm{O}\)):

\[ 1 \text{ mole of } \mathrm{C}_{3} \mathrm{H}_{8} \text{ produces } 4 \text{ moles of } \mathrm{H}_{2} \mathrm{O} \]

Step 3: Calculate the Moles of Water Produced

Given that we have 7.60 moles of propane, we use the mole ratio to find the moles of water produced:

\[ 7.60 \text{ moles of } \mathrm{C}_{3} \mathrm{H}_{8} \times \frac{4 \text{ moles of } \mathrm{H}_{2} \mathrm{O}}{1 \text{ mole of } \mathrm{C}_{3} \mathrm{H}_{8}} = 30.40 \text{ moles of } \mathrm{H}_{2} \mathrm{O} \]

Final Answer

\[ \boxed{30.40 \text{ moles of } \mathrm{H}_{2} \mathrm{O}} \]

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