Honors Chemistry Test Chapter 11 (write rest tomrrow)

Absolute zero

Colder temperature does not exist and no motion possible and its is zero kelvin

Atmosphere (atm)

Most common unit of pressure is atmosphere (atm) the average pressure at sea level

Avogadro’s law

The Volume of a gas and the amount of the gas in moles (n) are directly proportional. Assumes constant temperature and pressure.

Boyle’s Law

Law assumes constant temperature and a constant number of gas particles. The volume of a gas and its pressure are inversely proportional.

Charles’s Law

Law assumes constant pressure and a constant amount of gas. The volume of a gas and its kelvin temperature are directly proportional.

Combined Gas Law

For a sample of gas under two different sets of conditions, we use combined gas law.

Dalton’s law of partial pressures

The sum of the partial pressures of each component in a gas mixture must equal the total pressure as expressed by Dalton’s law of partial pressures

Hypoxia

Low oxygen levels can have a negative physiological effects called hypoxia or oxygen starvation. Causes dizziness and headaches and shortness of breath.

Ideal gas constant (R)

We can replace proportional sign with equal sign by adding R a proportionality constant.

Ideal gas law

Contains simple gas laws and shows how other pairs of variables are related.

Kinetic molecular Theory

• A gas is a collection of particles in constant, straight-line motion.

• Gas particles do not attract or repel each other they do not interact. The particles collide with each other and with the surfaces around them; then they bounce back like idealized billiard balls.

• There is a lot of space between gas particles compared with the size of the particles themselves.

• The average kinetic energy—energy due to motion—of gas particles is proportional to the temperature of the gas in kelvin. This means that as the temperature increases, the particles move faster and therefore have more energy.

• Gases are compressible.

• Gases assume the shape and volume of their container.

• Gases have low densities in comparison with liquids and solids.

• Gases are compressible because there is so much empty space between gas particles.

• Liquids are not compressible because there is so little space between the liquid particles.