Tires are one of the most frequently encountered applications of the gas laws that we never think about. We fill our tires with air, or with nitrogen, but it always works out the same way. Enough gas goes in, the tire inflates, and then the pressure starts going up. In this assignment, we’ll be investigating the ways that the gas laws impact how we treat our tires. Even outside of the Fast series, people havediscussed bizarre modifications to tires andtheir gases in the interest of speed, such asreplacing regular air with helium!Determine how many moles of gas particlesare in your tire, if your tire pressure gaugereads 2.31 atm on a sunny 26.0 °C day. Thevolume of your average tire is 10.50 L. Whatis the total mass of the gas in your tire if it isair (MW of air = 28.96 g/mol)?What is the total mass of the gas if it ishelium instead?Write one short sentence about whether youthink the mass difference would besignificant enough for consideration for aFormula 1 race. I have good information that in Fast 29,Dominic Toretto (Vin Diesel) will need torefill a tire quickly during a dramaticmoment. For this reason, he has a 3.00 Ltank of compressed air that is under2.7892*103 mmHg and is kept cool in dry iceat -35.0 °C.When Dom hooks his compressed air up tohis completely empty 10.50 L tire at 39.2 °Cand lets it run, what will his final tirepressure be, in atm? Assume all the air istransferred into the tire. Is his tire pressureabove the 2.31 atm that he needs to savethe planet/his family/his crew?

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Answered: Even outside of the Fast series, people…

Chemistry

10th Edition

ISBN:9781305957404

Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Chapter1: Chemical Foundations

Section: Chapter Questions

Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...

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Tires are one of the most frequently encountered applications of the gas laws that we never think about. We fill our tires with air, or with nitrogen, but it always works out the same way. Enough gas goes in, the tire inflates, and then the pressure starts going up. In this assignment, we’ll be investigating the ways that the gas laws impact how we treat our tires.

Even outside of the Fast series, people have
discussed bizarre modifications to tires and
their gases in the interest of speed, such as
replacing regular air with helium!
Determine how many moles of gas particles
are in your tire, if your tire pressure gauge
reads 2.31 atm on a sunny 26.0 °C day. The
volume of your average tire is 10.50 L. What
is the total mass of the gas in your tire if it is
air (MW of air = 28.96 g/mol)?
What is the total mass of the gas if it is
helium instead?
Write one short sentence about whether you
think the mass difference would be
significant enough for consideration for a
Formula 1 race.

I have good information that in Fast 29,
Dominic Toretto (Vin Diesel) will need to
refill a tire quickly during a dramatic
moment. For this reason, he has a 3.00 L
tank of compressed air that is under
2.7892*103 mmHg and is kept cool in dry ice
at -35.0 °C.
When Dom hooks his compressed air up to
his completely empty 10.50 L tire at 39.2 °C
and lets it run, what will his final tire
pressure be, in atm? Assume all the air is
transferred into the tire. Is his tire pressure
above the 2.31 atm that he needs to save
the planet/his family/his crew?

Definition Definition Any of various laws that describe the ways in which volume, temperature, pressure, and other conditions correlate when matter is in a gaseous state. At a constant temperature, the pressure of a particular amount of gas is inversely proportional with its volume (Boyle's Law) In a closed system with constant pressure, the volume of an ideal gas is in direct relation with its temperature (Charles's Law) At a constant volume, the pressure of a gas is in direct relation to its temperature (Gay-Lussac's Law) If the volume of all gases are equal and under the a similar temperature and pressure, then they contain an equal number of molecules (Avogadro's Law) The state of a particular amount of gas can be determined by its pressure, volume and temperature (Ideal Gas law)

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