Gases- HONORS

Kinetic Molecular Theory

• Describes the behavior of an ideal gas

• Explains the properties of solids

• Details the structure of atoms

• Analyzes chemical reactions

A real gas deviates (differs) from an ideal gas because:

• Real gases have a small, but significant volume

• Real gases have no volume at all

• Real gases are always in a gaseous state

• Real gases do not interact with each other

Gases behave most like an ideal gas under the following conditions:

• low temperature

• high pressure

• high temperature

• low pressure

Volume vs. Temperature

• 
• Volume decreases with temperature in solids

• Volume remains constant with temperature changes

• Volume is independent of temperature in liquids

Graham's Law of Effusion states that at the same conditions of temperature and pressure, the lightest gas will effuse (diffuse) most rapidly. Which of the following statements is true according to Graham's Law?

• The heaviest gas will effuse most rapidly.

• At different temperatures, gases effuse at the same rate.

• At the same conditions of temperature and pressure, the lightest gas will effuse most rapidly.

• Gases effuse at a rate proportional to their molecular weights.

What is the Ideal Gas Law?

• @@PV = nRT@@

• @@P = rac{nRT}{V}@@

• @@V = rac{nRT}{P}@@

• @@n = rac{PV}{RT}@@

Pressure vs. Volume

• 
• Pressure and volume are directly proportional.

• Pressure is independent of volume.

• Volume increases as pressure increases.

STP

• Standard Temperature and Pressure

• Standard Time and Pressure

• Standard Temperature and Power

• Standard Time and Power

The 2 gases that behave most like an ideal gas

• Hydrogen

• Helium

• Oxygen

• Nitrogen

Dalton's Law of Partial Pressure

• The total pressure of a mixture of gases is equal to the sum of the partial pressures in the mixture.

• The total pressure of a gas is equal to the pressure of the gas at absolute zero.

• The total pressure of a gas is independent of the number of gas particles present.

• The total pressure of a gas is equal to the average kinetic energy of the gas particles.