Jump to: navigation, search

Boyle's law


<include></include>

Lesson: 133
Unit: 4
State Content Standard: 4c

Lesson Title: Boyle's Law
Textbook Page: Pages 403-407, 415, 435
Chemistry Passport: Page 147


Objectives
1. Understand the relationship between pressure and volume.
2. Complete calculations involving this law.


Lesson Content

In Boyle's law, there is a pressure to volume relationship. Specifically, there is an inverse relationship between the pressure and volume of a gas with a fixed mass. According to this gas law, volume increases as pressure decreases and volume decreases as pressure increases.<ref>http://www.grc.nasa.gov/WWW/K-12/airplane/boyle.html</ref>

Boyle's law can be represented by the following equation: P1V1=P2V2
(Only for identical masses of gas at constant temperature.)<ref>Zumdahl, Steven S., Susan L. Zumdahl, and Donald J. DeCoste. World of Chemistry. Boston: Houghton Mifflin Company, 2006. Print.</ref>

To Solve Calculations...

1. List.

P1=
V1=
P2=
V2=

2. Plug it in.

P1V1=P2V2

3. Does your answer make sense? (Remember to check your units!)


Diagram


Example Problems

1. Under what circumstance might a gas decrease in volume when heated?

A. The gas is held constant at STP.
B. The gas remains under uniform temperature.
C. The gas is placed under increasing pressure.
D. The gas undergoes a decrease in pressure.

2. If the volume of a gas-filled container increases, what happens to the pressure?

The pressure decreases.

3. If the air pressure in a room drops but the temperature remains constant, what happens to a filled balloon?

The balloon expands. (Its volume increases.)

4. A gas occupies 12.3 L at a pressure of 40.0 mm Hg. What is the volume when the pressure is increased to 60.0 mm Hg?

(40.0 mm Hg)(12.3 L)=(60.0 mm Hg)(x) --> x=8.20 L

5. If a gas at 25.0°C occupies 3.60 L at a pressure of 1.00 atm, what will be its volume at a pressure of 2.50 atm?

(1.00 atm)(3.60 L)=(2.50 atm)(x) --> x=1.44 L


State Released Test Question

The volume of 400 mL of chlorine gas at 400 mm Hg is decreased to 200 mL at constant temperature. What is the new gas pressure?

A. 400 mm Hg
B. 300 mm Hg
C. 800 mm Hg
D. 650 mm Hg

How to Solve the Calculation:

1. List.

P1=400 mm Hg
V1=400 mL
P2=x
V2=200 mL

2. Plug it in.

P1V1=P2V2
(400 mm Hg)(400 mL)=(x)(200 mL)
x=800 mm Hg

3. Does your answer make sense? (Remember to check your units!)

The pressure was doubled, while the volume was halved.


References

Unknown extension tag "references"



Suggested Readings

http://www.universetoday.com/73852/boyles-law/


Download Lesson

(Flipchart) | (Flipchart PDF) | (PPT) | (MS-Word) | (PDF)


Continue to Next Lesson: Charles' Law



Do you see an error on this page? Please create an account and help us edit this page. Your help is greatly appreciated.