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silverwasp255Lv1

23 Apr 2020

(a) Amonton’s law expresses the relationship between pressure and temperature. Use Charles’s law and Boyle’s law to derive the proportionality relationship between P and T. (b) If a car tire is filled to a pressure of 32.0 lbs/in.² (psi) measured at 75 °F, what will be the tire pressure if the tires heat up to 120 °F during driving?
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Beverley SmithLv2

26 May 2020

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If a car tire is filled to a pressure of 31.5 lbs/in2 (psi) measured at 72 âF, what will be the tire pressure if the tires heat up to 118 âF during driving?

Part 1 Boyle’s Law P1 V1 = P2 V2 when Temperature is constant; being 1 “initial” and 2 “final” A container of oxygen gas has a volume of 150 mL when its pressure is 0.947 atm. If the temperature remains constant. What will the volume of the gas be at a pressure of 0.987 atm? Using Boyle’s Law solve for V2 of final volume using P1 V1 = P2 V2 Match the correspondent given data, unknown data and resulted in data after solved

___1. Initial Volume or V1

___2. Final Pressure or P2

___3. Initial pressure or P1

___4. Final V2

___5 Temperature

A. does not change, remains constant

B. 144 mL of oxygen

C. 0.947 atm

D. 150 mL of oxygen

E. 130 mL of oxygen

F. 0.987 atm

Part 2 Charles’s Law V1/T1=V2/T2 when the Pressure is constant; being 1 “initial” and 2 “final A container with hydrogen gas has a volume of 349 mL, at a temperature of 22.0C (Change to K), What volume will the gas occupy at 50C(Change to K), if the pressure remains constant?

____6. Final Volume of gas

____7 Initial Temperature gas

____8. Final Temperature gas

____9. Initial Volume gas

____10. The pressure of hydrogen

G. It’s constant

H. 295 K

I. 349 mL

J. 382 mL

K. 323 K

L. 50 C

Part 3 Gay-Lussac Law P1/T1=P2 when the volume (V) is constant A cylinder of a gas has a pressure of 4.40 atm at 25C (Change to K). At what temperature in Celsius will it reach a pressure of 6.50 atm C= K-273

____11. Final Pressure of gas (P1)

____12. The initial temperature in K (T1)

____13. The initial Pressure of gas (P2)

____14. The volume of the gas

_____15. The final temperature of the gas

M. 6.50 atm

N. 298 K

O. 4.40 atm

P. 167 C

Q . 283 K

R. is constant

Part 4 Combined Gas Law P1 V1/ T1 = P2 V2/ T2 OR MORE EASY TO SOLVE P1 V1 T2= P2 V2 T1 A St. Valentine Helium-filled balloon for your love, has a volume of 50.0 mL at 25 C (change to K) and 1.08 atm. What volume(V2) will it have at 0.855 atm and 10.0C (change to K). K=C + 273

_____16. The Final Temperature in K (T1)

_____17. The initial Volume in mL (V1)

_____18. The final Pressure in atm (P2)

_____19. The initial temperature in C (T1)

_____20. The final volume (V2)

S. 298k

T. 50.0 mL

U. 0.855 atm

V. 25 C

W. 283 K

X. 60.00 mL

Part 5 Answer with the letter in the blank. A. Boyles’s Law B. Charles’s Law C. Gay-Lussac’s Law D. Combined Gas Law E. Avogadro’s Law

___21. One mol of any gas at Standard Temperature and Pressure contains 6.03 X10^23 molecules and occupy a volume of 22.4L

____22. The higher the pressure the lower the volume when the temperature is constant.

____23. The higher the temperature the higher the volume when the pressure is constant.

____24 The higher the temperature the higher is the pressure when the volume is constant.

____25. There is a relation between pressure, volume, and temperature of a fixed amount (moles)of gas

coffeeelephant81

Calculate the volume of air within a typical bicycle tire (or, if you like, choose an atypical tire size that you prefer). This calculation does not need to be precise: A reasonable approximation would be the volume of a cylinder with the radius of the inner tube and the length of its circumference.

(b) Calculate the number of moles of air molecules in the inflated tire. For this calculation, it is reasonable to treat the air as an ideal gas and use the gas constant with units of atmospheres for pressure and liters for volume: R = 0.08206 L Â· atm Â· K â1molâ1 Assume that the temperature is 300 K, and be sure to indicate the final pressure that you are assuming. What is the initial volume of the air at atmospheric pressure?

(d) How would you go about filling the tire with the minimum amount of work? What conditions would you maintain during this process? What is the minimum amount of work required?

(e) If you have much experience with this activity, you probably know that the temperature of the air is likely to increase as you fill the tire. Why does the temperature increase? How would you expect the temperature increase to affect the amount of work that you have to do? (f) Suppose that you have just eaten a candy bar. How many tires must you pump up to work off the nutritional energy of the candy bar, assuming that 10% of the candy bar calories are converted to work (and the rest to metabolic heat)? Also assume that the temperature of the air remains constant and that you use the minimum amount of work to pump up each tire. Be careful: nutritional information is usually reported in âbig Câ calories, which is the amount of energy required to raise the temperature of 1 Kg of water by 1 â¦C, not 1 g.

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