Final answer:
To determine the number of CO2 molecules produced from the combustion of 3.5 liters of C4H6, you need to balance the chemical reaction, convert liters to moles using the ideal gas law, and then apply stoichiometry and Avogadro's number to convert from moles to molecules of CO2.
Step-by-step explanation:
To calculate the number of molecules of carbon dioxide produced when 3.5 liters of C4H6 combusts, you first need to know the balanced chemical equation. Assuming complete combustion, each molecule of C4H6 would react with O2 to form CO2 and H2O. The balanced equation for the combustion of butadiene (C4H6) would look something like this:
2C4H6 + 11O2 → 8CO2 + 6H2O
We see that 2 moles of C4H6 produce 8 moles of CO2. In this step, we apply Avogadro's number (6.022 × 10^23 molecules/mole) to convert moles to molecules. Next, since the ideal gas law states that one mole of gas at standard temperature and pressure occupies 22.4 liters, we can calculate the number of moles of C4H6 in 3.5 liters:
Number of moles of C4H6 = Volume / Molar volume = 3.5 L / 22.4 L/mol
Then, using the stoichiometric relationship, we will multiply the moles of C4H6 by the ratio of CO2 produced per C4H6 from the balanced equation (8 moles of CO2 per 2 moles of C4H6).
Finally, we calculate the number of co2 molecules by multiplying the moles of CO2 by Avogadro's number. Without providing the numerical answer due to the requirement, the student can now perform the calculations to find the number of CO2 molecules.