gases Flashcards
four gaseous properties
- moles (n)
- pressure (p)
- volume (v)
- temperature (T)
moles
- the amount of gas in a particular sample, in moles
volume
- the amount of space a gas sample occupies (the volume of its container)
- usually in L
pressure
- force exerted over an area: the frequency and force of collisions in a gaseous system btwn particles and the container
- atm, KPa, and torr
- 1 atm: 760 torr/mmHg, 101 KPa
kinetic energy (KE)
- the energy associated with the velocity of an object
temperature
- measure of the average KE of the sample
- temperature up, particles’ avg velocity up, pressure up in a rigid container/volume up in a fluid container
- measured in C, but calculate in K
- C + 273 = K
internal pressure
outward pressure on the inner walls of a container, caused by collisions between gas molecules in the sample and the walls
external pressures
inward pressure on the outer walls of the container caused by atmospheric pressure
temperature
the average kinetic energy of the center of mass of the gas sample
kinetic molecular theory
is based on the idea that matter is composed of tiny particles that are always in motion and helps explain observable properties and behaviors of gases
KMT postulate 1
gas particles move in continuous, random motion
KMT postulate 2
the volume of gas particles is negligible compared to the volume of the container
KMT postulate 3
attractive & repulsive forces between as particles are also negligible (no IMF)
KMT postulate 4
under constant temperature, there is a constant KEL perfectly elastic collisions (no energy is lost)
KMT postulate 5
the average KE of particles is proportional to the absolute temperature in K
