1.7 Kinetic Theory
Learn
Practice Test
Spaced Repetition
Match
Flashcards1/25
There's no tags or description
Looks like no tags are added yet.
Name | Mastery | Learn | Test | Matching | Spaced |
|---|
No study sessions yet.
26 Terms
what is the definition of a gas?
a state of a substance which expands to fill any volume that it is placed in
what are 4 examples of thermodynamic, measurable quantities?
pressure, temperature, volume, number of moles
what is pressure?
the force experienced on one unit area of surface in contact with the gas
what is temperature?
a measure of the average kinetic energy of the particles in the gas
what is temperature measured in?
kelvin
what is volume?
a measure of the total space occupied by the gas
what are moles?
a measure of the number of particles in the gas, 1 mol = 6.02 Ă—1023 particles
what is boyle’s law?
when temperature is constant, pressure is inversely proportional to volume
what is charles’s law?
when pressure is constant, volume is proportional to temperature
what is the pressure law?
when volume is constant, pressure is proportional to temperature
what is the value of the boltzmann constant?
1.38 Ă— 10-23
what does N stand for?
the total number of particles
what does NA stand for?
Avogadro’s Number
what does n stand for?
the number of moles
what is the relative molecular mass?
the mass of a molecule, relative to 1/12th that of Carbon-12
what is molar mass?
the mass per mole
how can we calculate the molar mass?
relative molecular mass / 1000
what does the ideal gas equation describe?
a gas which has a number of properties that real physical gasses do not have
what are the properties of an ideal gas?
no intermolecular forces
the size of particles is negligible compared to the volume of gas
the collisions between particles are perfectly elastic
the motion of particles is purely random
what is no intermolecular forces equivalent to saying?
the particles only carry kinetic energy
when can we approximate a real gas to behave like an ideal gas?
when the temperature is large and the pressure is small
why cant a gas be ideal if its pressure is too large?
the potential energy associated with the distance between particles will become more significant compared to their kinetic energy
what is pressure caused by?
collisions between the particles and container walls
what is force?
the rate of change of momentum
what is the average kinetic energy of a gas particle proportional to?
the temperature of the gas