Gas Laws

Gases generally have

• low density

• high density

• closely packed particles

• no increase in volume when temperature is increased

• no decrease in volume when pressure is increased

Pressure is

• defined as the mass that an object exerts when at rest

• measured in Newtons

• defined as the number of moles of substance divided by the mass of the substance

• defined as the force per unit area

• measured in grams

Boyle's law states that:

• Equal amounts of gases occupy the same volume at constant temperature and pressure.

• The volume of a fixed amount of gas is inversely proportional to its pressure at constant temperature.

• The volume of a fixed amount of gas is directly proportional to its temperature in Kelvin at constant pressure.

• The total pressure of a mixture of gases is the simple sum of the partial pressure of all of the gaseous compounds.

• The rates of effusion of gases are inversely proportional to the square roots of their molar masses.

Avogadro's law states that:

• Equal amounts of gases occupy the same volume at constant temperature and pressure.

• The volume of a fixed amount of gas is inversely proportional to its pressure at constant temperature.

• The volume of a fixed amount of gas is directly proportional to its temperature in Kelvin at constant pressure.

• The total pressure of a mixture of gases is the simple sum of the partial pressure of all of the gaseous compounds.

• The rates of effusion of gases are inversely proportional to the square roots of their molar masses.

Charles's law states that:

• Equal amounts of gases occupy the same volume at constant temperature and pressure.

• The volume of a fixed amount of gas is inversely proportional to its pressure at constant temperature.

• The volume of a fixed amount of gas is directly proportional to its temperature in Kelvin at constant pressure.

• The total pressure of a mixture of gases is the simple sum of the partial pressure of all of the gaseous compounds.

• The rates of effusion of gases are inversely proportional to the square roots of their molar masses.

Consider a sample of helium gas in a container fitted with a piston, as pictured below. The piston is frictionless, but has a mass of 10.0 kg. How many of the following processes will cause the piston to move away from the base and decrease the pressure of the gas? Assume ideal behavior.

I. heating the helium

II. removing some of the helium from the container

III. turning the container on its side

IV. decreasing the pressure outside the container

• 0

• 1

• 2

• 3

• 4

Tags

NGSS.HS-PS3-4

A gas sample is held at constant pressure. The gas occupies 3.62 L of volume when the temperature is 21.6°C. Determine the temperature at which the volume of the gas is 3.42 L.

• 312K

• 278K

• 20.4K

• 295K

• 552K

A balloon has a volume of 2.32 liters at 24.0°C. The balloon is heated to 48.0°C. Calculate the new volume of the balloon.

• 2.32L

• 2.51L

• 2.15L

• 4.64L

• 1.16L

Body temperature is about 309 K. On a cold day, what volume of air at 276 K must a person with a lung capacity of 2.2L breathe in to fill the lungs?

• 2.46L

• 1.97

• 2.08

• 3.93

You are holding four identical balloons each containing 10.0 g of a different gas. The balloon containing which gas is the largest balloon?

• H₂

• He

• Ne

• O₂

• All have the same volume.