Unit 8 (chapter 13) Flashcards
Absolute temperature
amount of gas
Avogadro’s number
Boyle’s law
Charles’ law
When the amount and pressure of a gas are held constant, the volume and Kelvin temperature are directly proportional
Combined Gas Law
Dalton’s Law
For a mixture of gases in a container, the total pressure exerted is the sum of the partial pressures of the gases present
Gay-Lussac’s Law
When the amount and volume of a gas are held constant, the pressure and Kelvin temperature are directly proportional
ideal gas
a gas that follows the kinetic molecular theory completely
Ideal Gas Law
kinetic molecular theory
A set of rules on how we expect gases to behave
- Gases consist of very small particles that are far apart relative to their size (mostly empty space)
- Gas particles are in constant, random motion. The moving particles constantly collide with each other and the walls of the container
- Collisions between gas particles and container walls are elastic collisions
- There are no forces of attraction or repulsion between gas particles (will not clump or repel because they’re moving too fast)
- The average kinetic energy of gas particles depends on the gas temperature (hotter = faster)
partial pressure
the pressure that the gas would exert if it were alone
pressure
standard pressure
air pressure of dry air at sea level
standard temperature
273K
temperature
volume
kinetic energy
energy anything has if it’s moving. moving faster means more energy
Average kinetic energy is directly proportional to Kelvin temperature
solids kinetic energy
very little
liquids kinetic energy
more than solids
gases kinetic energy
lots, in constant motion. 1000mph at STP
Inelastic collisions
kinetic energy disappears (ex: slime balls hitting each other)
Elastic collisions
Bounces right back, no kinetic energy waster (ex: rubber balls hitting each other)
Expandability
If an open container had gas, the fas would leave the container and fill any given area (unique to gases)
Diffusion
The process of gases moving around (ex: movie theater popcorn smell filling a mall) (unique to gases)
Compressibility
Because there’s so much empty space in gases, you can squeeze them into very small spaces (unique to gases)
SI unit for pressure
Pa
Atmospheric pressure & gravity
atmospheric pressure changes with elevation (gravity)
conversion factors (mm Hg)
1 standard atmosphere = 1.000 atm = 760.0 mm Hg = 760.0 torr
conversion factors (Pa)
1 standard atmosphere = 101,325 Pa
conversion factors (psi)
1.000 atm = 14.69 psi
To fully describe a gas…
you need to know
- temperature (T)- K or °C (standard T=273K)
- volume (V)- L or mL
- pressure (P)
- amount (n)- mol
Avogadro’s Law
for a gas at a constant temperature and pressure, the volume is directly proportional to the number of moles
