Ideal Boyles Lussac Charles Gas Laws Ideal Boyles Lussac Charles

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

Gas Laws

Boyles Law =Temp is Constant

Lussac’s Law= Volume Constant

Charles Law= Pressure Constant

Combined Gas Law

1. A 550.0 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?

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

3. A gas has a pressure if 0. 0370 atm at 50. 0C 3. A gas has a pressure if 0.0370 atm at 50.0C. What is the pressure at standard temperature?

Ideal gas law

Ideal Gas Law PV =nRT R = gas constant R = 8.31 LkPa R= 0.0821 Latm moleK moleK R= 62.4 mmHg L all other units can mole K be converted

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.  

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. 0.425 moles of ammonia gas (NH3) at 10.5 PSI and 37C.

6. Determine the amount: answer: 0.51g a. In moles, of 1.25L of O2 at 805.6 mmHg and 250K. b. In grams, of 0.80L of ammonia gas at 0.925 atm and 27C. answer: 0.51g

Ok now your turn to practice: Answers 7) 26.6 L 10) 111 PSI 8) 30L 11) 318 K 9) 2.22 L 12) 3.1 x 104 L Don’t forget: 1 atm= 760mmHg(torr)=101.3kPa=14.7psi °C= 5/9 (°F-32)