at what state do elements or compounds have their greatest kinetic energy
gases
pressure
the force of collisions per unit area of the surface
what are the 4 basic physical properties of a sample of gas
pressure
volume
temperature
number of moles
what does the simple gas law describe
how all 4 properties of a gas each relate to volume because it is the easiest to measure
Boyles law ad the equation
relationship between pressure and volume is an inverse relationship
(smaller volume means gas collides with surface more often)
P1V1=P2V2
Charles law and the equation
relationship between volume and temperature is a linear relationship
(when temp increases, gas move faster, colliding with surface more often)
V1/T1=V2T2
Can the temp go below 0K, if not why
no, its at absolute zero and if K becomes negative then volume will as well, which is impossible
Avogadro’s Law and equation
relationship between volume and amount is linear.( when add more gas, gas collide more often)
V1/n1=V2/n2
according the avogadros law what happens when pressure stays constant when adding more gas
volume must increase
according to Charles’ law as temp increase and external pressure remains constant what happens to the tires
volume increases
according to Boyle’s law what happens when volume decreases
pressure increases
what is the ideal gas law
combination of Boyle’s, Charles’, and Avogadro’s laws as they all relate to Volume
what are the units of R and the constant
0.08206 Latm/molK
what is the volume of an ideal gas at stp
22.4 L
trait of STP
1 atm and 0 Celsius
what does density allow us to do
relate molar mass to the ideal gas law
in ideal gas do the gases interact
no, they can be treated separately in equations
kinetic molecular theory
gas is a collection of particles in constant motion
a single particle moves in straight line until it collides with another or surface of container.
what is the first assumption for ideal gas law
particle size is negligible
particles occupy no volume
what is the second assumption of ideal gas law
average kinetic pressure of a particle is proportional to temperature
all particles are moving, not equally
higher temp means more average kinetic energy.
are kinetic energy and velocity the same
no
what is the third assumption of ideal gas law
collision of one particle with another is completely elastic
they exchange energy
exert no force on each other
what happens when far away from STP to gases
they don’t act as ideal gases because the assumptions break down
what are the corrections for assumption 1
gas particles do actually have a defined volume
molar volume is higher than predicted by ideal gas law at high pressure
