CHEM 130 Chapter Notes - Chapter 8: Ideal Gas Law, Gas Constant, Ideal Gas

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1 Apr 2017

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A gas uniformly fills any container, is easily compressed, and mixes completely with any other gas; gases exert pressure on their surroundings. Barometer is a device used to measure atmospheric pressure: atmospheric pressure results from the mass of air being pulled toward the center of the earth; gravity, atmospheric pressure varies with altitude. Taken together, boyle"s, charles"s, and avogadro"s laws can combine to form the ideal gas law: pv = nrt, where r is the universal gas constant, which changes depending on the units. Ideal gas law is an equation of state for a gas where the state of the gas is its conditions at a given time; based on experimental measurements of properties of gases. Molar volume is the volume of one ole of an ideal gas; @ stp, it is 22. 4 l. Standard temperature & pressure (stp) for gases stp conditions are 1 atm and 0 c; common reference conditions for properties of gases.

Related Questions

To understand several methods of measuring gas pressure. Gases exert a measurable pressure (P) on the walls of their container. The SI unit for pressure is the pascal (Pa). Other pressure units frequently used in chemistry are millimeters of mercury (mmHg) and atmospheres (atm). You can convert between units of pressure using conversion factors such as those indicated below. 1 atm=760 mmHg=101,325 Pa

Part A

On a rainy day, a barometer reads 737 mmHg . Convert this value to atmospheres.

Express your answer numerically in atmospheres

Part B

A closed container is filled with oxygen. The pressure in the container is 445 kPa . What is the pressure in millimeters of mercury?

Express the pressure numerically in millimeters of mercury.

Part C

What is the pressure (in atmospheres) of the gas inside the container connected to an open-end, mercury-filled manometer as shown in the picture? (Figure 1) The atmospheric pressure is 0.95 atm.

Express your answer numerically in atmospheres.

1. Convert 0.955 atm to kPa:

A) 96.8 kPa

B) 96.8 x 103 kPa

C) 96.765 kPa

D) 96.77 kPa

2. Consider a manometer where the height of the mercury column is 32 mm higher on the atmospheric side than on the gas side. If the laboratory pressure is 1 atm, what is the pressure of the gas in the manometer?

A) 792 torr

B) 732 torr

C) 760 torr

D) 728 torr

E) 766 torr

F) 97000 Pa

3. If a balloon is cooled, the volume _______ while the pressure inside the balloon _________

A) increases, remains the same

B) decreases, increases

C) decreases, remains the same

D) decreases, decreases

4. The following are commonly observed properties of gases (There may be more than one answer):

A) gases do not exert pressure on surroundings

B) gases experience a "memory" effect and take on the shape of previous containers

C) gases have no definite shape of their own

D) gases cannot be compressed

E) a gas completely fills the container it occupies

F) gases exert pressure on their surroundings

G) gases are highly compressible

Thank you!

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

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CHEM 130 Chapter Notes - Chapter 8: Ideal Gas Law, Gas Constant, Ideal Gas

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