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Set up the dimensional analysis problem to determine how many moles of carbon dioxide will form when 98.2 grams of propane react with oxygen. Refer to the periodic table.

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.


Learn more about combustion of propane here:

https://brainly.com/question/3014094


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