ch 10

solids, liquids and gases

the strongest intermolecular forces and a fixed volume shape

a weaker intermolecular force and takes the shape of the container but not volume

Fills the entire container (volume) takes the shape Intermolecular forces are very weak Lowest density of matter Particles do not interact much with each other

describes the behaviour of ideal gases

K

T (in K)= T(in C + 273.15)

Pressure= Force/Area

1 ideal gases are in constant, random motion and move in straight lines 2 the volume of a volume gas is considered to be zero 3 They are elastic 4 There are no intermolecular forces (they dont attract or repel each other) 5 Temperature is directly proportional to the average kinetic energy of the gas particle

Any gas behaves ideally in low pressures and high temperatures

They would be large and have more intermolecular forces to each other. They would react less with the walls and result in a decrease of pressure

Over time the particles would hit the walls with less force and there would be a decrease in pressure

1 Pa = 1N/m^2

1 atm=1bar

more particles=larger volume volume in gas is directly proportional to the number of moles in the gas

Vn=k, where V is the volume of the gas, n is the number of moles of the gas, and k is a proportionality constant.

higher pressure, smaller volume

P1V1=P2V2 where mols and temperature are constant

The higher the temperature the larger the volume

V₁ / T₁ = V₂ / T₂, where V₁ and T₁ are the initial volume and temperature, respectively. Similarly, V₂ and T₂ are the final values of these gas parameters. Where mols and pressure are constant

The ideal gas law PV=nRT P=atm V=L T=K