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When temperature decreases, pressure decreases and vice versa (balloon) (P1/T1 = P2/T2)
Gay Lussac’s Law
Moles increase & Volume increase
Avogadro’s Law
When temperature increases, volume increases (balloons) V1/T1 = V2/T2) *temperature is always on the bottom except for boyle’s law and that one’s inverse
Charles’ law
When pressure increases, volume decreases (think peeps or like when walls close in on someone)
Boyles’ Law (only inverse relationship)
P1V1/T1= P2V2/T2
combined gas law
1 atm = 101.3 kPa = 760 mmHg = 760 torr= 14.7 psi 32 F = 0 C = 273 K
conversions
Particles move in random straight line motion
KInetic molecular theory
The volume of a fixed amount of gas to constant pressure is directly proportional to absolute temperature V1/T1 = V2/T2
charles’ law
gas has no volume/volume is neglectable, particles are separated by a great distance (spaced out), gas particles have NO ATTRACTION
properties of gas by kinetic molecular theory
gas particles have no attraction and will collided with each other against the wall of their container or each other, which can result in a transfer of energy but no net loss of energy from those collisions
gas properties by kinetic molecular theory
What is the average kinetic energy of the gas particles?
not all particles have the same energy, but the avergage kinetic energy of the gas particles are their temperature
when does a gas behave like an ideal gas?
low temperature and high pressure (think of soda)
V1/T1 = V2/T2
Charles’ Law (volume, temperature)
P1V1= P2V2
Boyles’ Law (pressure, volume)
P1/T1 = P2/T2
Gay lussac’s law (pressure, temperature)
V1/N1 = V2/N2
Avogadro’s Law