Honors Chem Chapters 10, 11, and 12. Kinetic Molecular Theory (KMT) Molecules are constantly in motion and collide with one another and the wall of a.

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Presentation transcript:

Honors Chem Chapters 10, 11, and 12

Kinetic Molecular Theory (KMT) Molecules are constantly in motion and collide with one another and the wall of a container Particles move faster with increased temperature Gases are made of mostly empty space and just a few fast moving particles.

Properties of Gases Low Density Expansion Compressibility Fluidity Diffusion/Effusion

Nature of Gases Diffusion: spontaneous mixing of gases

Nature of Gases Effusion: gas particles spontaneously pass through a small opening

Graham’s Law of Diffusion (or Effusion) Smaller, lighter gas molecules move faster through the air than larger, heavier gas molecules. “Lighter, faster, farther”

Graham’s Law of Diffusion (or Effusion)

Graham’s Law: Rewritten r = rate MM= Molar Mass d = distance t = time light = lighter gas heavy = heavy gas

Kinetic Molecular Theory (KMT) Molecules are constantly in motion and collide with one another and the wall of a container Particles move faster with increased temperature Gases are made of mostly empty space and just a few fast moving particles.

Ideal Gas Ideal Gas: a gas that perfectly conforms to assumed gas behavior (doesn’t exist) Most gases are described using real conditions and variables

Variables of Gases (P) Pressure (V) Volume (T) Temperature (n) Amount of gas in moles

Pressure Measures: Force exerted by moving gas particle collisions with their container

Pressure Units Units: 1 atm (atmosphere) of pressure is the average pressure at sea level Important Conversions: 1 atm= 760 mmHg (millimeters of Mercury) = 760 torr = kPa (kilo Pascals) = 14.7 psi (pounds per square inch)

Volume Measures: amount of space that a gas occupies Units: Liters (L) Important Conversions: 1 L = 1000mL

Temperature Measures: average kinetic energy of gas particles. Units: Kelvin (K) The Celsius scale is NOT used for gases because gases can still have kinetic energy at negative and 0 o C.

Kelvin Scale and Absolute Zero Absolute Zero = 0 Kelvin represents the temperature at which a gas has NO kinetic energy

Converting Temperature Important Conversions: o C = K K – 273 = o C

STP STP = Standard Temperature and Pressure Exactly 0 o C and 1 atm At STP, one mole of gas (6.02 x10 23 particles) occupies 22.4 L If a gas is not held at STP, then volume is recalculated

Gas Variables A variable is a factor that is liable to change. Pressure, temperature, and volume of a gas are liable to change. Pressure, volume, and temperature are interdependent. When variable changes, they all do.

The Combined Gas Law Relates pressure, temperature, volume, and moles of a gas Relates initial and final conditions Variables that do not change are constants and not included in the equation

The Combined Gas Law Equation The left side (1) represents the initial conditions of the gas The right side (2) represents the final conditions of the gas

Charles’ Law: Volume and Temp What changes? And How? Volume increases, temperature increases What stays the same? Pressure and moles are held constant (toss ‘em)

Charles’ Law: Equation Remember: Temperatures must be in Kelvin

Charles’ Law: Graph Direct Relationship: both variables increase together

Charles Law: Simulation

Charles’ Law: Video Demo

Charles’ Law : Example A gas sample at 25 o C and 752 mL is heated to 50 o C, what is the new volume?

Boyle’s Law : Pressure and Volume What changes? And How? When Pressure increases, Volume decreases What stays the same? Temperature and moles are held constant (toss ‘em)

Boyle’s Law : Equation Remember: Pressure units on both sides of the equation must be the same P 1 V 1 = P 2 V 2

Boyle’s Law: Graph Inverse Relationship: an increase in one variable with a simultaneous decrease in the other

Boyle’s Law: Simulation

Boyle’s Law: Video Clip

Boyle’s Law Example Q: A 1.0 L sample of gas is held at standard pressure, 1.0 atm. The pressure of the gas is reset to 152 mmHg. What is the new volume of the gas?

Gay-Lussac’s Law: Pressure and Temperature What changes? And how? As temperature of a gas increases, the pressure also increases What stays the same? Volume and moles are held constant (toss ‘em)

Gay-Lussac’s Law: Equation Pressure units on both sides of the equation must be the same Temperature must be in Kelvin

Gay-Lussac’s Law: Graph Direct Relationship: Both variables increase together

Gay-Lussac’s Law: Simulation

Gay-Lussac’s Law: Video Clip

Gay-Lussac’s Law: Example Q: A gas has a pressure of atm at 50.0 °C. What is the pressure at standard temperature?