Module 12 Flashcards
State Charlie’s Law
under conditions of constant pressure, the temperature and volume are linearly proportional to each other
TEMP AND VOLUME PROPORTIONAL
Define boiling point
the temperature at which the liquid’s vapor pressure is equal to atmospheric pressure.
VAPOR PRESSURE EQUAL TO ATMOSPHERIC PRESSURE
pressure
the force per unit area exerted on an object P= F/A
Pascal (Pa)
the pressure unit of Newtons/ square m
1.000 atm =
- 3 kPa
- 0 torr
- 0 mmHg
Boyle’s Law
as long as the temperature of a gas stays the same, the product of the gas’ volume and its pressure is always the same PV= constant
GAS VOLUME AND PRESSURE IS SAME WITH A CONSTANT TEMP
Absolute temp scale
kelvin temp scale that can never reach 0 degrees
Extrapolation
following an established trend in the data even though there is no data available for that region
combined gas law
PV/ T = constant (p- pressure, v-volume, t- temp)
When using any equation in this module, I must always use
the Kelvin Temp scale
Ideal gas
a gas that applies to the combination gas law
three properties of an ideal gas
molecules/atoms that make it up are very small compared to the total volume available to the gas
MOLECULES SMALL COMPARED TO TOTAL VOLUME
molecules/atoms that make it up are so far apart from one another that there is no attraction or repulsion between them
MOLECULES WITH NO ATTRACTION/REPULSION
the collisions that occur between the gas molecules/atoms must be ELASTIC COLLISIONS
elastic in terms of this module
when molecules/ atoms collide with each other or the walls of the container, no energy is lost
Standard temp and Pressure (STP)
a temp of 273 K and a pressure of 1.00 atm
used as a reference to determine whether or not a gas is ideal
A gas with a temp that is … and a pressure that is… will behave in an ideal fashion.
close to (or larger than) 273 K near (or lower than) 1.00 atm
Daltons law of Partial Pressures
when ideal gases are mixed, the total pressure of the mixture is equal to the sum of the pressures of each individual gas Pt = P1 + P2 + P3 + …
(Pt= total pressure) (P1, P2 etc are referred to as PARTIAL PRESSURES)
The pressure of an ideal gas does not depend on the … It depends only on the…
identity of the gas
quantity of that gas
vapor pressure
the pressure exerted by the vapor which sits on top of any liquid
the vapor pressure of any liquid …
increases with increasing temp
mole fraction
X = # of moles of component/ total # of moles in the mixture
