How many grams of CO2 are produced from the complete combustion of 1 mole of C3H

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Question: How many grams of CO2 are produced from the complete combustion of 1 mole of C3H8?

Options:

Correct Answer: 88 g

Solution:

C3H8 + 5O2 → 3CO2 + 4H2O. 1 mole of C3H8 produces 3 moles of CO2. Mass = 3 * 44 g = 132 g.

How many grams of CO2 are produced from the complete combustion of 1 mole of C3H8?

How many grams of CO2 are produced from the complete combustion of 1 mole of C3H8?

Step 1: Write the balanced chemical equation for the combustion of propane (C3H8). The equation is C3H8 + 5O2 → 3CO2 + 4H2O.
Step 2: Identify how many moles of CO2 are produced from 1 mole of C3H8. From the equation, 1 mole of C3H8 produces 3 moles of CO2.
Step 3: Calculate the mass of CO2 produced. Each mole of CO2 has a mass of 44 grams.
Step 4: Multiply the number of moles of CO2 by the mass of one mole of CO2. So, 3 moles of CO2 * 44 grams/mole = 132 grams of CO2.

Stoichiometry – Understanding the mole ratios in chemical reactions to calculate the amount of products formed from a given reactant.
Molar Mass Calculation – Calculating the mass of a substance using its molar mass and the number of moles produced.