1. AP Chemistry Notes
Chapter 5: Gasses

2. 5.1 Pressure Pressure is defined by force/area P=F/A
Standard pressure = pressure at sea level
Units for pressure at standard pressure
1 Atm = 760 torr =760 mmHg = kPa = 101,325 Pa
These equivalents are given to you on the AP Exam
Temperature and volume effect pressure

3. 5.1 Example, Conversion between units of pressures

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5. 5.2 The Gas Laws of Boyle and Charles
Boyle’s Law
Used when temperature does NOT change
P (pressure) is inversely proportional to V (volume)
P1V1 =  P2V2
Charles Law
Used when pressure does NOT change
(P) Pressure is proportional to (T) temperature
V1/T1= V2/T2
Temperature HAS to be measures in Kelvin

6. 5.2 example, using Charles/Bolyes Law

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8. 5.3 The Ideal Gas Law
We know that when measuring pressure temperature and volume won’t always stay so then we use the ideal gas law.
PV=nRT where R is a constant of
R = L · atm/mol · K

9. 5.3 example, using the Ideal Gas Law

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11. 5.3 example, using the Ideal Gas Law in variable changes

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13. 5.4 Gas Stoichiometry Simply put 1 mole of any gas is 22.42L
Given to you on AP exam

14. 5.4 example, Gas stoichiometry
I have 1 mole of a gas at 273K and 1 atm, what volume of gas do I have?

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16. 5.4 example, Gas stoichiometry

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18. 5.5 Dalton’s Law of Partial Pressures
Often there a lot of different gasses in a container
thus we must use Dalton’s Law of Partial Pressures to calculate how much of each gas there it
Ptotal = P1+P2+P3
Each number is a different gas in that container
Use one of the gas laws to calculate each pressure

19. 5.5 example, Using Dalton’s Law of Partial Pressures

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21. 5.5 example, Using Dalton’s Law of Partial Pressures

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23. Learn! Multiple Choice Questions Based on these

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