Final answer:
When 1.7 moles of O2 react completely according to the balanced equation for the combustion of propane, they produce 1.02 moles of CO2.
Step-by-step explanation:
The question asks how many moles of carbon dioxide (CO2) are produced when 1.7 moles of oxygen (O2) react completely according to the balanced chemical equation for the combustion of propane (C3H8). The balanced equation for the reaction is:
C3H8 + 5O2 → 3CO2 + 4H2O
From the balanced equation, we can see that 5 moles of O2 are required to produce 3 moles of CO2. This sets up a stoichiometric ratio of CO2 to O2 as 3:5. To find out how many moles of CO2 are produced from 1.7 moles of O2, we can set up the following calculation:
(1.7 moles O2) * (3 moles CO2 / 5 moles O2) = 1.02 moles CO2
Therefore, when 1.7 moles of O2 react completely, 1.02 moles of CO2 are produced.
From the balanced equation C3H8 + 5O2 ➨ 3CO2 + 4H2O, we can see that 1 mole of propane reacts with 5 moles of oxygen to produce 3 moles of carbon dioxide. Therefore, to find the number of moles of CO2 molecules produced when 1.7 moles of O2 react completely, we can set up a proportion:
5 moles of O2: 3 moles of CO2 = 1.7 moles of O2: x
By cross multiplying, we get:
5x = 1.7 * 3
x = 1.7 * 3 / 5
x ≈ 1.02 moles of CO2