KMT and gas laws, KMT & Gas Laws

Boyle's Law

As pressure increases, volume decreases

Charles' Law

As temperature increases, volume increases

p1v1=p2v2

formula for boyle's law

v1/t1=v2/t2

formula for charles' law

p1v1/t1=p2v2/t2

formula for combined gas law

PV=nRT

formula for ideal gas law

The pressure will increase because the heated gas increases the overall average kinetic energies of the molecules. When the molecules are heated up and have higher average kinetic energy, the molecules will move faster, thus hitting the rigid container more frequently, resulting in an increase of pressure. Or, you can look at it from PV=nRT, according to this formula, you can see that pressure is proportional to temperature. So if temperature goes up, pressure will go up (V, n, and R are held constant)

Enclosed gas in rigid (lidded) container. What happens when you heat it + why?

collisions with gas particles on the walls of a container

What makes pressure?

Expandability

a gas will expand to take the shape of whatever container it is in. This agrees with kinetic molecular theory because gas particles move randomly in all directions, and there are no attractive or repulsive forces between particles

Fluidity

A gas had the ability to flow. This agrees with KMT because there are no attractive or repulsive forces between gas particles which might prohibit their ability to flow and because gas particles are in constant, rapid, random motion.

Low Density

The density of a gas is about 1/1000 the density of the same substance in the liquid state. This agrees with KMT because the particles are so much farther apart in the gaseous state.

Compressibility

the volume of a given sample of gas can be greatly decreased. This agrees with KMT because of the large amount of space between gas particles, and so they can be pushed closer together.

Diffusion and Effusion

Gases spread out and mix with one another, even without being stirred. This agrees with KMT because of the constant, random motion of gas particles.

evaporation

phase change, liquid to gas

condensation

phase change, gas to liquid

sublimation

phase change, solid to gas

deposition

phase change, gas to solid

freezing

phase change, liquid to solid

melting

phase change, solid to liquid

kinetic molecular theory (motion)

matter is composed of particles that are in constant motion

kinetic molecular theory (attraction)

there are forces of attraction between particles that depend on the distances between particles

kinetic molecular theory (temperature)

the higher the temperature, the faster the particles move

ideal gas conditions

high temperature, low pressure, low molecular mass

kelvin scale

degrees C + 273

Charles' law

pressure held constant, direct relationship

Boyle's law

temperature held constant, indirect relationship

Gay-Lussac's law

volume held constant, direct relationship

law of partial pressure

all the partial pressures add up to the total pressure