Shared Flashcard Set

Details

Gas Stoichiometry
Basic laws, concepts, and etc. of gases.
41
Chemistry
11th Grade
06/01/2011

Additional Chemistry Flashcards

 


 

Cards

Term
Gay-Lussac's Law
Definition
P1T2=P2T1 directly proportional
Term
Charles's Law
Definition
V1T2=V2T1 directly proportional
Term
Boyle's Law
Definition
P1V1=P2V2 inversely proportional
Term
Combined Gas Law
Definition
P1V1T2=P2V2T1 amount of gas does not change
Term
Ideal Gas Law
Definition
PV=nRT
Term
Standard Temperature & Pressure
Definition
273K and 1.00 atm
Term
Amount of Atmosphere Gases
Definition
80% N2,20% O2, and trace amounts of CO2, H20, and Argon
Term
Pressure
Definition
force per unit area
p=f/a
lower as you go up
Term
Barometer
Definition
glass tube with mercury, inverted and held in dish of mercury. Atmosphere supports 1 meter tall of mercury.
Term
What are the units of pressure equal to STP?
Definition
1.00 atm
101325 Pa
101.325 kPa
14.7 psi
760. mm Hg
760. torr
Term
1 Pascal equals...
Definition
1 N/m2
Term
Dalton's Law of Partial Pressures
Definition
each gas exerts it's own pressure, not affected by other gases in the mixture and each individual pressure is called the partial pressure.
P total = Pa + Pb + Pc
Term
Mole fraction
Definition
sum of the moles of each of the gases divided by each gases's individual moles and is expressed as an percent and can multiply by the pressure to get the partial pressure.
Term
Collected over water gases
Definition
MUST subtract the partial pressure of the vapor from the original pressure to find the pressure of the gas.
Term
Real Gas Behaviors
Definition
High Pressure (not much room), and low temperature (slow)
Must consider volume of particles
If conditions are extreme enough, may change into liquid
Term
Ideal Gas Behaviors
Definition
High temperature (fast), low pressure (a lot of room)
Term
Kinetic Energy Theory
Definition

KE= 1/2 mv2

1)Gases consist of tiny particles, atoms, or molecules 2) Volume of gas particle is irrelevant compared to the entire sample 3) Gas particles are in constant, random motion 4) No retractive/repulsive forces (move too fast) 5) When heat increases, then velocity, kinetic energy and average kinetic energy increases

Term
Properties of Gases
Definition
They flow, transmit & exert pressure equally in all directions, in constant & random motion, collisions are elastic (no loss of kinetic energy), mostly empty space, no free sides, and collisions with walls = pressure.
Term
Laws
Definition
Laws show what happens, so we can make predictions, theories try to explain why.
Term
Temperature
Definition
average kinetic energy and is constant during a phase change
Term
Avogadro's Law
Definition
a gas at a constant temperature and pressure has a volume directly proportional to the number of moles of gas
Term
proportionality constant
Definition
.08206 atm L/ mole K
Term
molar volume
Definition
1 mol/22.40 L at STP
Term
Condensation
Definition
gas to liquid
Term
Deposition
Definition
gas to liquid
Term
Freezing
Definition
liquid to solid
Term
Melting
Definition
solid to liquid
Term
Sublimation
Definition
solid to gas
always occurs below the triple point
Term
Vaporization
Definition
liquid to gas
occurs at specific temperature
occurs at the bottom
based on vapor pressure and atmospheric pressure
Term
Diffusion
Definition
movement of one material through another
Term
Triple Point
Definition
temperature and pressure at which all three phases exist
Term
What happens to the density of a gas as it is compressed?
Definition
It become more dense because there is less room with the same amount of particles present.
Term
Critical Point
Definition
temperature and pressure at and above which vapor and liquid are the same
Term
Boiling Point
Definition
temperature at which the vapor pressure of a liquid is equal to the external pressure
Term
Evaporation
Definition
liquid to gas below boiling point
occurs at the surface
based on vapor pressure of liquid
Term
Normal Boiling Point
Definition
temperature at 1.00 atm at which something boils
Term
Melting Point
Definition
increase the pressure, decrease the melting point
Term
Vapor Pressure
Definition
closed container of water and air water evaporates into vapor until above liquid is saturated with vapor at point of saturation, the vapor condenses back into a liquid at the same rate the liquid evaporates
Term
Dynamic Equilibrium
Definition
reversible processes at the same rate
Term
As vapor pressure increases...
Definition
temperature increases, evaporation increases, number of particles increases, and collisions increase
Term
What do air pockets do for water?
Definition
Makes it taste better
Supporting users have an ad free experience!