Ch. 8 Flashcards
based on the kinetic-molecular theory states what four things about gases? a gas with these characteristics is called what?
- space between molecules is so small, it has no volume
- molecules in constant motion and collision of molecules against container walls is pressure of gas
- molecules experience no intermolecular forces
- Avg KE is proportional to absolute temp
A GAS WITH THESE THINGS IS AN IDEAL GAS
what is formula to find K from C
K=C+273.15
pressure can use what units
1 atm=760 torr=760mmHg
what is standard temp and pressure
its NOT STANDARD CONDITIONS
temp is 0C, pressure is 1 ATM, and 1 mol of gas is 22.4 L
what is charles law
if pressure is constant than volume is proportional to temp, gas will expand when heated and vice versa
what is boyles law
if temp is constant than pressure is inversely proportional to volume. increase volume causes more space to move therefore decreasing pressure
if volume is constant than what is pressures relationship with temp
pressure is proportional to temp
what are some deviations from ideal gas behavior
- pressure of real gases is smaller than if gas was ideal (because more interactions b/w molecules not walls)
- volume of real gas is smaller than if gas was ideal (because volume occupied by gas is no longer negligible)
what conditions of pressure and temp causes ideal deviations
high pressure and low temp
what is total pressure
this is due to the collisions of all types of molecules within containers
what is partial pressure
the pressure exerted by one type of gas in the overall pressure of all gases within a container
what is daltons law of partial pressures
total pressure is sum of partial pressures of all constituent gases
what is effusion
escape of a gas molecule through a hole into an evacuated region
what is rate of effusion based on
based on weight of molecule since heavier molecules take longer to move
what is gas constant
0.083 L-atm/K-mol
a barometer with a liquid less dense than mercury would have the same, more, or less reading compared to a barometer with mercury
it would have a higher reading because the liquid would need to reach higher in the column for it to be equal at the pressure of the atmosphere
with constant n and p, what is ideal gas formula?
v1/t1=v2/t2
with constant n and t, what is ideal gas formula?
p1v1=p2v2
with constant n and v, what is ideal gas formula?
p1/t1=p2/t2
what is combined gas law? what value needs to stay constant
n needs to be constant for the formula to be p1v1/t1=p2v2/t2
what is avogadros law
if equal volume containers have same pressure and temp, then they contain same number of particles
what is avogadros formula
V1/n1=v2/n2
what is standard molar value? what conditions must be met before you use this?
SMV is 22.4 L and temp must be 273 and pressure 1 atm
how can you tell if a gas will deviate from ideal gas behavior
any gas that interacts with other molecules, increased IMF, will deviate because ideal gases have zero IMF
how can you tell if a gas will more likely act as an ideal gas
if its small, most likely not polyatomic, zero to weak IMF
what conditions cause ideal gases to deviate?
high pressure and low temp
what conditions causes ideal gas law to give similar results as to real gas?
high temp and low pressure because these conditions allow molecules not to get close to each other
gas in the same container may have different speeds but they will always have the same
temperature or kinetic energy
molecule 1 is .6 grams and molecule 2 is .2 grams, which molecule will still be in a container with a small hole in it
molecule 1 because it weighs more having a slower effusion
what is grahams law of effusion?
square root of molar mass of gas b divided by molar mass of gas A, first molecule always at bottom
how would you calculate molar ratio
- balance equation, 2. you divide moles of specific compound by total moles on its specific side (reactants or products)
partial pressure is proportional to
total number of moles of a gas
