NAME: If your car gets 21.4 mpg, how many lbs of CO, will you release into the a

Question

NAME: If your car gets 21.4 mpg, how many lbs of CO, will you release into the atmosphere, if you drove the 1280 miles from Towson University to Key West Florida for a much needed break after taking a summer chemistry course? neud What volume of O2 is if the barometric pressure is 732 torr and it is 78 Assume that gasoline is 100% octane; therefore the following reaction should considered. 818(1)+ IS Physical Constants that you will find necessary: Density of octane = 0.7025 g/ml 1 Gal 3.79L 1LB = 454 g

Explanation / Answer

Volume of octane used = distance / cars average

= 1280 miles / 21.4 mpg

= 59.813 gallon x 3.79 L / gal

= 226.69 L

Mass of gallon used = density x volume

= 0.7025 g/mL x 226.69 L x 1000mL/L

= 159249.725 g

Moles of octane used = mass/molecular weight

= 159249.725 g / 114.23 g/mol

= 13949.52 mol

From the stoichiometry of the reaction

2 mol octane produces = 16 mol CO2

13949.52 mol octane produces = 16*13949.52/2

= 111596.09 mol CO2

Mass of CO2 released = moles x molecular weight

= 111596.09 mol x 44 g/mol

= 4910228.201 g x 1lb/454g

= 10815.48 lb

Part b

Moles of O2 required

= 25 mol O2 x 13949.52 mol octane / 2 mol octane

= 174369 mol O2

Volume of O2 = moles x R x T / P

= 174369 mol x 0.0821 L-atm/mol-K x (78+273)K / (732/760) atm

= 5217014.71 L x 1 gal / 3.79 L

= 1376521.03 gallon

Related Questions

Navigate

• Browse (All)
• Browse N
• Subjects

---

---

Integrity-first tutoring: explanations and feedback only — we do not complete graded work. Learn more.