I. Gas Laws A. Four properties of gases 1. Volume - V

Gas Laws

Learning Objectives TLW know the variables that influence the behavior of gases (TEKS 9) TLW be able to describe interrelationships between temperature, number of moles, pressure, and volume of gases in an enclosed system (TEKS 9.A) TLW perform stoichiometric calculations to determine mass and volume relationships between reactants and products involving gases (TEKS 9.B) TLW describe the postulates of kinetic molecular theory (TEKS 9.C)

I. Gas Laws A. Four properties of gases 1. Volume - V gases do not have a defined volume particles of a gas expand to fill their container volume is measured in L (liters) 2. Pressure P collisions of particles with a surface P measured in atm, kpa, torr, mm Hg

3. Temperature T the measure of average particle speed or kinetic energy gas particles are in constant motion T o for gases are measured in K (Kelvin) 4. Quantity n measure of how much there is of a gas MOLES!!!!! 22.4 L of gas = 1 mole

Postulates of Kinetic Molecular Theory Gases are composed of a large number of particles that behave like hard, spherical objects in a state of constant, random motion. These particles are much smaller than the distance between particles. Most of the volume of a gas is therefore empty space. There is no force of attraction between gas particles or between the particles and the walls of the container. These particles move in a straight line until they collide with another particle or the walls of the container. Collisions between gas particles or collisions with the walls of the container are perfectly elastic. None of the energy of a gas particle is lost when it collides with another particle or with the walls of the container. The average kinetic energy of a collection of gas particles depends on the temperature of the gas and nothing else.

Postulates of Kinetic Molecular Theory Check out this interactive tool which demonstrates the postulates in action http://www.chm.davidson.edu/vce/kineticmol eculartheory/basicconcepts.html

B. Gas laws are based mathematically on the relationship of the four properties of gas volume pressure temperature quantity

II. The Gas Laws (4 major ones) A. Boyle s Law 1. Discovered that gas pressure and volume are related 2. If pressure is increased then volume decreases 3. Pressure and volume are inversely related 4. Meaning = whatever pressure does volume does the opposite

NASA Video

Boyle s Law P 1 V 1 = P 2 V 2 P V

V 2 = 2.1 L 5. Example of Boyle s Law A sample of gas has a volume of 4.2 L and a pressure of 0.95 atm. If the pressure on the balloon increases to 1.90 atm what will the new volume be? 0.95 atm 1.90 atm P 1 V 1 = P 2 V 2 4.2 L V =? (.95 atm)(4.2l) = (1.90 atm)v 2

B. Charles Law 1. Discovered the relationship between volume and temperature 2. If T o increases then the volume increases 3. T o and volume are directly proportional 4. Meaning = whatever volume does T o does the exact same thing

NASA Video

Charles Law V 1 /T 1 = V 2 /T 2 V NOTE: All T o must be Kelvin!!!! T o C + 273 = K

V 2 = 2.54 L KELVIN!!!!!!!! 5. Example of Charles Law Another sample of gas has a volume of 2.0 L and a T o of 100 o C. If the T o is increased to 200 o C, what will the new volume be? V = 2.0L V =? V 100ºC 200ºC 1 /T 1 = V 2 /T 2 2.0L/(100 o C + 273) = V 2 /(200 o C + 273)

C. Gay-Lussac s Law 1. Discovered the relationship between Pressure and T o 2. If T o increases then Pressure increases 3. T o and P are directly proportional 4. Meaning = whatever T o does pressure does the exact same thing

Gay-Lussac s Law P 1 /T 1 = P 2 /T 2 P T

Example of Gay-Lussac s Law Another sample of gas has a volume of 2.0 L a T o of 25 o C, and a pressure of 2.00 atm. If the T o is increased to 75 o C, what will the new pressure be? 2.00 atm P =? P 1 /T 1 = P 2 /T 2 V = 2.0L 25ºC V = 2.0L 75ºC 2.00 atm/(25 o C + 273) = P 2 /(75 o C + 273) P 2 = 2.34 atm

D. Avogadro s Law If pressure and temperature are kept constant, the volume of a gas is directly proportional to number of moles of a gas This is why a balloon gets larger as you blow it up not the pressure 1 mole of gas = 22.4 L Mathematically speaking.. V 1 = V 2 n 1 n 2

Example of Avogadro s Law I have a balloon with 0.25 moles of air in it and its volume is 0.30 L. If I blow it up more to 0.75 L, how many moles have I added of air? V 1 /n 1 = V 2 /n 2 0.30 L = 0.75 L = 0.63 moles 0.25 moles n 2 moles

E. Combined Gas Law 1. Sometimes the pressure (P in atm, kpa, torr, mm Hg), temperature (T in K), volume (V in L), and/or moles (n for number) change 2. So must combine formulas from all four dudes. 3. Looks like this P 1 V 1 = P 2 V 2 T 1 n 1 T 2 n 2

Example of combined gas law 8.0L of neon gas at 23 o C and 900 mm Hg is then compressed to 2.0 L and the T o is raised to 225 o C. What will the new P be? n is constant P V /T n = P V /T n 1 1 1 1 2 2 2 2 (900 mm Hg)(8.0 L)/(23 ºC + 273) = P 2 (2.0 L)/(225 ºC + 273) P = 6057 mm Hg 2

F. Ideal Gas Law PV = nrt R = ideal gas constant 0.0821 L atm mol K 8.31 L kpa mol K 62.4 L mmhg mol K

Web Exploration ASPIRE Animation Activity (link) Gas Law Investigation (link) Data Collection Sheet (link)

Khan Academy Tutoring on Gas Laws