CHM-1045 Lecture Notes - Lecture 8: Combined Gas Law, Ideal Gas Law, Kinetic Theory Of Gases

97 views2 pages

ultramarinefrog201

17 Nov 2017

School

FSU

Department

Chemistry and Biochemistry

Course

CHM-1045

Professor

Cameroun Robert

For unlimited access to Class Notes, a Class+ subscription is required.

Document Summary

Gas pressure is the result of the force of gas molecules when colliding with the surfaces of objects. 760 mm hg = 760 torr = 1 atm = 101325 pa. Gay-lussac"s law. the pressure is directly related to temperature with constant volume. Volume is directly related to temperature with constant temperature. Volume is inversely related to pressure with constant temperature. Mole of a gas is directly related to its volume with constant pressure and temperature. v1/n1=v2/n2 ideal gas law. A relation between the pressure, volume, temperature, and number of moles of a gas: R value= 0. 08206 l atm mol 1 k 1 and 8. 314 kpa l mol 1 k 1. Ideal gas happen under low pressure and high temperature. Spreading of gas molecule into surface area. Rate of diffusion= amount of gas passing through an area /unit of time. The escape of molecule through hole (cid:2870)= (cid:3050)(cid:2870) (cid:2869)

Related Questions

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

A sample of nitrogen gas in a 1.94-L container exerts a pressure of 1.54 atm at 21 âC.What is the pressure if the volume of the container is maintained constant and the temperature is raised to 344 C?

The volume of the container is held constant. Pressure is directly proportional with temperature. Use the pressure-temperature law.

P1 / T1 = P2 / T2

P1 = 1.54 atm
T1 = 21Â°C (301K)
T2 = 344Â°C (605K)

Asked: P2 (what is the final pressure when the temperature is increased? Expect a higher final pressure).

*** convert Celsius temperatures to Kelvin by adding 273.

Derive the formula for P2.

P2 = P1T2 / T1
= (1.54)(605) / 344
= 2.708 atm (this is the worng answer) Please help

Charlesâs law states that the volume of a gas is directly related to the absolute temperature when there is no change in the pressure or amount of gas: (Figure 1)

V1T1=V2T2

Part A

A sample of gas in a balloon has an initial temperature of 30 âC and a volume of 1770 L . If the temperature changes to 90 âC , and there is no change of pressure or amount of gas, what is the new volume, V2, of the gas?

Express your answer with the appropriate units.

Part B

What Celsius temperature, T2, is required to change the volume of the gas sample in Part A (T1 = 30 âC , V1= 1770 L ) to a volume of 3540 L ? Assume no change in pressure or the amount of gas in the balloon.

Express your answer with the appropriate units.

Show transcribed image text

CHM-1045 Lecture Notes - Lecture 8: Combined Gas Law, Ideal Gas Law, Kinetic Theory Of Gases

Document Summary

Get access

Related Documents

CHM-1045 Lecture Notes - Lecture 10: Mean Free Path, Kinetic Theory Of Gases, Exothermic Reaction

CH 301 Lecture Notes - Lecture 2: Torr

CHEM 1320 Chapter Notes - Chapter 5: Fluorine, Effusion

Related Questions