Answer :
Final answer:
To find the moles of carbon dioxide formed from 98.2 grams of propane, we first convert the mass of propane to moles using its molar mass, which is approximately 44.094 g/mol. Then, using the balanced reaction, we find that 1 mole of propane produces 3 moles of carbon dioxide. Therefore, 98.2 grams of propane will yield approximately 6.69 moles of CO₂.
Explanation:
Dimensional Analysis for the Reaction of Propane
To determine how many moles of carbon dioxide (
CO₂) will form when 98.2 grams of propane (
C₃H₈) react with oxygen, we can follow these steps:
Step 1: Write the Balanced Equation
The balanced chemical equation for the combustion of propane is:
C₃H₈(g) + 5O₂(g) → 3CO₂(g) + 4H₂O(g)
Step 2: Calculate Moles of Propane
First, we need to convert grams of propane to moles. The molar mass of propane is calculated as follows:
- Carbon (C): 12.01 g/mol 3 = 36.03 g
- Hydrogen (H): 1.008 g/mol 8 = 8.064 g
Thus, the total molar mass of propane is:
36.03 g + 8.064 g = 44.094 g/mol
Now, we can find the number of moles of propane in 98.2 grams:
moles of C₃H₈ = 98.2 g / 44.094 g/mol = 2.23 moles (approximately)
Step 3: Use Stoichiometry to Find Moles of CO₂
Using the balanced equation, we can see that:
3 moles of CO₂ are produced for every 1 mole of C₃H₈ reacted.
So, the moles of CO₂ produced from 2.23 moles of propane would be:
2.23 moles C₃H₈ * (3 moles CO₂ / 1 mole C₃H₈) = 6.69 moles CO₂
Therefore, around 6.69 moles of CO₂ will be produced when 98.2 grams of propane combust.
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