Gases Flashcards
Relationship of gas particles
space between particles is greater than the size of the particles themselves
What is the gas particles motion
translational kinetic energy (a straight line)
as the temperature increases
the gas gains more kinetic energy
property of their particle collision
elastic (no energy is lost)
what do we assume in a gas
they behave ideally, where the particles have no IMF with one-another, and the mass and size of the gas particles are negligible
compressibility
highly compressible
- a gas can fit into various sizes of containers
EMPERICIAL PROPERTIES
properties that are measurable using scientific instruments
THEORETICAL PROPERTIES
assumptions as to the behaviour of gas on a particles level based on its empirical properties
what are the empirical properties of gas
- VOLUME (V)
- PRESSURE (P)
- TEMPERATURE (T)
- AMOUNT (n)
VOLUME (V)
3D space that contains gas
- L or mL
IL = ? ml
1000
PRESSURE (P)
when gas particles collide with the walls of the container, the frequency of the collisions and the speed of the collisions produces a measurable force
- kPa, Pa
1 kPa = ? Pa
1000 Pa
BAROMETER
instrument used to measure presssure
? atm = ? kPa = ? mmHg = ? torr
1 atm = 101.325 kPa = 760 mmHg = 760 torr
TEMPERATURE (T)
measure of the average kinetic energy of the particles of a substance
- celsius or kelvin
ABSOLUTE ZERO
extrapolated theoretical lowest temperature possible for any substance. No molecular movement
0 K = -273.15 C
C = ? K
K: C + 273
C: K - 273
AMOUNT (n)
of particles present in the gas sample
- mol
GAY-LUSSAC’S LAW
temperature and pressure of a gas are directly proportional provided that volume and chemical amount are kept constant
BOYLE’S LAW
pressure of a gas varies indirectly with its volume at constant temperature and chemical amount
what will happen to the pressure if V dec.
pressure with inc. proportionately
what will happen to the pressure if V inc.
pressure with dec. proportionately
what will be shown on the graph for the pressure volume relationship
inverse curve
as V approaches 0, what happens to P
becomes infinitely high
as P approaches 0, V become ?
infinitely high
why does V dec. and pressure inc.
space between the particles dec., inc. collisions more frequently, and resulting in high pressure
formula for BOYLE’S LAW
P1V1V = P2V2
CHARLES LAW
temperature (in K) and volume of a gas are directly proportional, at constant pressure and chemical amount
graph for temperature and volume
linear (direct relationship)
why does the graph SLOWLY inc.
different IMF’s, high IMF = slow reaction
intial properties in charles law
high kinetic energy, low IMF
final properties in charles alw
low kinetic energy, IMFs’ can develop, particles come closer together (dec. V)
formula for CHARLES LAW
V1/T1 = V2/T2
STP
standard temperature and pressure
- 0 C and 101.325 kPa
SATP
standard ambient temperatures and pressure
- 25 C and 100 kPa
formula for GAY-LUSSACS
P1/T1 = P2/T2
overall formula for boyles, charles, and gay-lussacs law
P1V1/T1 = P2V2/T2
