Question

For the reaction shown, calculate how many moles of each product form when the given amount of each reactant completely reacts. Assume there is more than enough of the other reactants.

C₃H₈(g) + 5O₂(g) yields 3CO₂(g) + 4H₂O(g)

Answer 1

To calculate the number of moles of each product formed when the given amount of reactant completely reacts, use stoichiometry. In this case, 0.602 mol of C₃H₈ reacts with 0.602 mol of O₂ to produce 1.806 mol of CO₂ and 2.408 mol of H₂O.

Step-by-step explanation:

The balanced chemical equation is C₃H₈(g) + 5O₂(g) → 3CO₂(g) + 4H₂O(g).

To calculate the number of moles of each product formed when the given amount of reactant completely reacts, we need to use stoichiometry.

Given that 13.5 L of O₂ is required to react with 2.7 L of C₃H₈, we can determine the ratio of moles between O₂ and C₃H₈. Using the ideal gas law, we know that 1 mole of any gas occupies 22.414 L at STP. Therefore, we can calculate the number of moles of O₂ as (13.5 L/22.414 L/mol) = 0.602 mol. Since the reaction is balanced at a 1:1 ratio between C₃H₈ and O₂, we can conclude that 0.602 mol of C₃H₈ is required.

Using the stoichiometric ratio from the balanced equation, we can determine the number of moles of CO₂ and H₂O produced. For every 3 moles of CO₂ produced, there are 4 moles of H₂O. Therefore, we have (3/1) × 0.602 mol = 1.806 mol of CO₂, and (4/1) × 0.602 mol = 2.408 mol of H₂O formed.