Chapter 6 Flashcards
(35 cards)
Kinetic Molecular Theory (KMT) of Gases - definition
gases consist of particles constantly moving through space in random directions and with various high-velocity speeds
How do single particles move according to the KMT?
in a straight line until they collide with something
According to the KMT, the average kinetic energy of gas particles is proportional to…
the temperature in Kelvin
collision of particles =
elastic
Elastic Definition
no net loss in kinetic energy
Pressure Definition
total amount of force exerted by gas molecules hitting a surface
Pressure Equation
P= force/area
How does gas pressure flow?
high to low pressure
The bigger the pressure difference…
the stronger the flow of gas
air pressure differences result in…
weather and wind patterns
higher altitude =
lower pressure
1 atm =
760 mmHg, 760 torr, and 14.7 lb/in^2 or psi
Boyle’s Law Equation
PV=K or P1V1=P2V2
Boyle’s Law Definition
when you decrease the volume of a container, more molecules will hit the wall at the same time, increasing the pressure
in Boyle’s Law as P increases…
V decreases by the same factor
Charles’ Law Definition
volume of gas is directly proportional to temperature
Charles’ Law Equation
V1/T1 = V2/T2
Charles’ Law Constants
P and n - pressure and amount of gas
Boyle’s Law Constants
T and n - temperature and amount of gas
Gay-Lussac Law Definiton
pressure is directly proportional to temperature
Gay-Lussac Law Equation
P1/T1 = P2/T2
Gay-Lussac Law Contansts
V and n - volume and amount of gas
Combined Gas Law Equation
(P1V1)/T1 = (P2V2)/T2
Combined Gas Law Constants
n - amount of gas
