welcome back.
let’s play a game of “some, none, or all” (flip me!)
i give you a statement, you tell me if that statement is true for all, some, or no gases
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"you have mass so you matter" - steward
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welcome back.
let’s play a game of “some, none, or all” (flip me!)
i give you a statement, you tell me if that statement is true for all, some, or no gases
gases are matter
all
gases are flammable
some
gases are visible
some
gases react
some (REMEMBER: noble gases!)
yay you did it! next section
hi
true or false: gases weigh differently depending on their molar mass
true!
how do gases move?
process called diffusion
why do gases move at different speeds?
what is the law that relates the speed of gases to their molar mass?
graham’s law
what are the four parts of kinetic molecular theory
gases…
are made of tiny particles, travelling in straight lines
do not occupy volume
collisions between molecules are perfectly elastic
no attractive or repulsive forces between the particles
temperature
measure of kinetic energy
volume
amount of space an object occupies
what determines volume for gases?
size of container
pressure
force of gas particles hitting the container
if particles are rapidly and frequently hitting the sides of the container, would the pressure be higher or lower?
higher
how does area affect pressure?
higher area → lower pressure
lower area → higher pressure
magic.
what is STP?
Standard Temperature & Pressure
now we get into the actual gas laws :D
yay
==Dalton’s Law==, what’s the tea?
==Dalton’s Law - Partial Pressure==
Example Problem: A mixture of 4.5% H2, 76% O2, and 19.5% N2 has a total pressure of 2.3 atm. What is the partial pressure of each of the gases?
PH2= 0.10 atm; PO2 1.75 atm; PN2= 0.45 atm
Next: @@Boyle’s Law@@
@@Boyle’s Law@@
what kind of container would gas have to be in to undergo @@Boyle’s Law@@?
flexible container (like a balloon) because the volume is changing
Example Problem: a gas occupies 1.65L at 1.00 atm what will be the new volume if the pressure becomes 3.00 atm?
0.520L
Charles’Law
Charles’Law
Example Problem: When 10.5 L of gas at 20C is heated, the volume increases to 21 L. What is the new temperature in Celsius? Assume no other changes in the gas.
313 C
%%Gay-Lussac’s Law%%
%%Gay-Lussac’s Law%%
When a gas has a pressure of 500 mmHg at 25C and is expanded to standard pressure, what happens to the temperature?
The temperature would rise to 452.96 K because the pressure and temperature are directly related
^^Combined Gas Law^^
^^Combined Gas Law^^
Ideal Gas Law
PV=nRT
what does the “R” stand for?
“R” → universal gas constant
what is the formula(s) to find molar mass?
M=m/n
\
M=dRT/P
how do you find density?
d=m/v