Module 6a: Gas Laws Flashcards
End Test 2
What does Kinetic Theory of Matter tell you?
A prediction of how matter should behave
T/F: All matter is made up of moving particles
T
Solids have tightly bound particles that ______
vibrate
Describe the particles in liquids
Free to move
still attracted to each other
Describe the particles in gases
Far apart
move freely
Phase changes occur with increases in ________ in matter
Kinetic energy
What form does kinetic energy normally come in?
Heat
What happens when you heat up a solid?
Particles can vibrate which increases entropy.
particles break apart and matter liquifies.
Continues to heat up. Can evaporate (turn into gas)
T/F: Physical properties of gases are all similar
T
Describe the boiling point of most gases?
Low
Gases are composed mainly of __________ elements with ________ formulas, ___________ compounds, and ________ molar masses
Nonmetallic
Simple
Small
Low
What are 3 additional characteristics of gasses
Expand to fill their container
highly compressible
extremely low densities
What happens when you compress and cool a gas?
Turns into a liquid
What type of mixture are 2 gases?
Homogeneous mixture
Describe the molecules in gases
Move independently
no forces keeping them together or pushing them apart
T/F: Kinetic Theory of Gases: Gases consist of large numbers of molecules that are in continuous, random motion
T
T/F: Kinetic Theory of Gases: Attractive and repulsive forces between gas molecules are strong
F
weak
When you increase the temperature, the kinetic energy goes ______
Up
T/F: Kinetic Theory of Gases: Energy can be transferred between molecules during collisons, but the average kinetic energy of the molecules does not change with time, as long as the temperate of the gas remains constant
T
T/F: Kinetic Theory of Gases: Average kinetic energy of gas molecules is dependent on a few factors
F
is ONLY dependent on the temperature
_________ is related to the average kinetic energy
temperature
u(rms) =
The root mean-squared speed
associated with average kinetic speed
T/F: At any given temperature, the average kinetic energy of molecules is the same
T
R =
0.08206
Temperature is measured in _______
Kelvin
Describe the relationship between molar mass and particle speed
Lower molar mass = higher speed
Higher molar mass = lower speed
Kelvin =
C + 273.15
What does STP mean?
Standard Temperature and Pressure
Temp = 273.15 Kelvin
Pressure = 1atm/760mmHg/760torr
Pressure Values:
1 atm = 760 mmHg = 760 torr
Pressure =
Force / Area
What is Atomospheric Pressure?
The weight of air per unit of area
What is the atomospheric pressure at sea level?
760 mmHg
Describe Gas Law: Boyle’s Law
P1V1 = P2V2
Pressure inversely related to Volume
Temp is constant
Decrease volume = increase pressure
Describe Gas Law: Charles’ Law
V1/T1 = V2/T2
Temp directly related to volume
Pressure and amount are constant
increase temp = increase volume
Describe Gas Law: Gay-Lussac’s Law
P1/T1 = P2/T2
Pressure is directly related to temp
Volume and amount are constant
increase temp = increase pressure
What gas law explains why water boils over at a lower temp at higher elevations?
Gay-Lussac’s Law
Describe Gas Law: Combined Gas Law
(P1V1)/T1 = (P2V2)/T2
Combination of Boyle’s, Charles’, and Gay-Lussac’s Law
n is constant
Describe Gas Law: Avogadro’s Law
V1/n1 = V2/n2
Volume directly related to moles
Temp and pressure are constant
increases moles = increased volume
At STP, how much volume does 1 mol of gas occupy?
22.4 L
n =
number of moles
Describe Gas Law: Ideal Gas Law
PV= nRT
R = 0.08206
Describe Gas Law: Dalton’s Law
If 2 gases that DO NOT REACT are combined in a container, ACT AS IF THEY ARE ALONE
Pt = P1 + P2 + P3…..
P1 = (n1/nt) x Pt
Describe Gas Law: Graham’s Law
r1/r2 = sq(M2/M1)
Relates molar mass of 2 gases to their rate of speed
decrease molar mass = increase rate of speed
What is effusion?
Escape of gas molecules through a tiny hole into an evacuated space until equilibrium is reached.
What is diffusion?
Spread of a substances through a space from a higher pressure to a lower pressure
Describe Gas Law: Henry’s Law
Solubility of a gas in a volume of liquid is porportional to partial pressure of that gas in equilibrium with that of the liquid
In the real world, the behavior of gases conforms to the ideal gas law only at ______ temperatures and ______ pressures
high
low
T/F: A gas will show different behaviors at high pressures and low temperatures
T
Gases need high temps and low pressures to be predictable
T/F: The assumptions of the Kinetic Theory of Gases are tue even when gases are exposed to low temperatures and high pressures
F
In the real world, this doesn’t work. This makes gas unstable.
Describe Gas Law: Van der Waals Equation
Takes into account ideal gas deviations
Adjustments include: Pressure and Volume
(P + N^2 a/V^2) (V-nb) = nRT
HE SAIDDDDDD HE WONT PUT THIS ON THE TEST
If we are to ASSUME a volume, what is it?
100ml
What is w/v?
(weight in grams) / 100ml !!!!!!!!!!!!!!!!!
What is w/w?
(weight in grams) / 100g !!!!!!!!!!!!!!!!!!!!!!!!!!!
