1. Ideal Boyles Lussac Charles
Gas Laws
Ideal
Boyles
Lussac
Charles

2. Variables that describe a Gas
P= Pressure T = Temperature (MUST be in Kelvin!) n= Amount (moles) V= Volume (MUST be in Liters!!)

3. Gas Laws

4. Boyles Law =Temp is Constant

5. Lussac’s Law= Volume Constant

6. Charles Law= Pressure Constant

7. Combined Gas Law

8. 1. A mL sample of nitrogen gas is warmed from 77.0C to 80.0C. Find the new volume if the pressure remains constant. What law does this situation follow?

9. 2. Convert 338L at 6.38 x 103 kPa to its new volume at standard pressure. What law does this situation follow?

10. 3. A gas has a pressure if 0. 0370 atm at 50. 0C
3. A gas has a pressure if atm at 50.0C. What is the pressure at standard temperature?

11. Ideal gas law

12. Ideal Gas Law
PV =nRT R = gas constant R = 8.31 LkPa R= Latm moleK moleK R= 62.4 mmHg L all other units can mole K be converted

13. 4. Calculate the pressure, in atmospheres, exerted by each of the following:
a. 250L of gas containing 1.35 moles at 320K
b. 4.75L of gas containing 0.86 moles at 300K.

14. 5. Calculate the volume, in liters, occupied by each of the following:
a. 4.0 grams of H2 at 300K and 1.25 atm.
b moles of ammonia gas (NH3) at 10.5 PSI and 37C.

15. 6. Determine the amount: answer: 0.51g
a. In moles, of 1.25L of O2 at mmHg and 250K.
b. In grams, of 0.80L of ammonia gas at atm and 27C.
answer: 0.51g

16. Ok now your turn to practice: Answers
7) L
10) 111 PSI
8) 30L
11) 318 K
9) L
12) 3.1 x 104 L
Don’t forget:
1 atm= 760mmHg(torr)=101.3kPa=14.7psi
°C= 5/9 (°F-32)