Chapter 7 (Gases) Flashcards
Gases
Boyle’s law
Volume is inversely related to pressure. (P1V1 = P2V2)
So as you increase the pressure you decrease the volume. This is at a constant temperature.
Charles’s law
Temperature and volume are proportional. (V1/T1 = V2/T2)
As you increase the temperature, you also increase the volume. This is at a constant pressure.
Ideal gas law
PV = nRT
P = pressure (atm)
V = volume (L)
n = number of moles
R = constant (0.08206 (L*atm)/(mol *K))
T = temperature (K)
Dalton’s law of partial pressures
The total pressure (P total) is equal to the sum of the partial pressures of all the gases in a mixture.
P total = P1 + P2 + …
Define standard temperature and pressure (STP).
Temperature = 273.15 K (0 C)
Pressure = 1 atm
Are gases low or high density? Why?
Low density; the molecules in a gas like to be far apart from each other and fill up the entire size of their container.
What are the seven diatomic elements?
H2, N2, F2, O2, I2, Cl2, Br2
(Have No Fear Of Ice Cold Beer)
What are the units of pressure?
Pressure is expressed as an amount of Force per Area:
P = F/A
What are units of pressure?
Pascal (Pa), atmosphere (atm), bar, torr, mmHg
What are the units of density?
Mass/Volume (m/V)
What is absolute 0 Kelvin?
Where volume = 0
Define standard molar volume.
It is the volume of 1 mole of an ideal gas at STP, which is 22.41 L
How many torr is in 1 atm?
760 torr
How many mmHg is in 1 atm?
760 mmHg
What is the mole fraction (X)?
mole fraction is a ratio of the amount of moles from one substance in a mixture, divided by the total number of moles.
What is the kinetic molecular theory of gases?
This describes the behavior of ideal gases.
What is Boltzmann distribution?
This states that not all gases move at the same speed or have the same kinetic energy. The distribution describes the different speeds and energies of different gases.
Define diffusion
This is the gradual mixing of two gases until the mixture is uniform.
Define effusion
This is a gas escaping from a tiny seep.
Graham’s law
The rate of effusion is inversely proportional to the square root of its molar mass.
