Gases Flashcards
(Gases) Relationship of torr (mm Hg) to atm
1 atm = 760 torr
(Gases) Pressure Equation
P=F/A
P — Pressure
F — Force
A — Area
(Gases) Kinetic Energy Equation
KE=0.5m(v^2)
m — mass
v — velocity
KE — kinetic energy
(Gases) Relationship of Kinetic Energy to Pressure
High KE = High P
Low KE = Low P
(Gases) Boyle’s Law
V₁P₁=V₂P₂
Increase V = Decrease P
xV=(1/x)P
USE WHEN TEMPERATURE AND MOLES ARE CONSTANT
(Gases) Charles’ Law
V₁/T₁=V₂/T₂
Increase V = Increase T
xV=xT
USE WHEN PRESSURE AND MOLES ARE CONSTANT
(Gases) Combined Gas Law
(P₁V₁)/T₁=(P₂V₂)/T₂
(Gases) Standard Temperature and Pressure of Gasses
0°C and 1 atm
(Gases) Avogadro’s Principle
There is the same number of gaseous particles in any given volume, given a constant pressure and temperature.
Ex. Two containers, one with 1 L He and another with 1 L H₂, have the same number of gaseous particles at 0°C and 1 atm.
(Gases) At STP, 1 mole of gaseous particles occupies ______ of space.
22.4 L
(Gases) Ideal Gas Equation
PV=nRT
P — pressure V — volume n — moles of gas R — Ideal Gas Constant (.0821) T — temperature (K)
(Gases) Molar Mass from Moles of Gas
mm=m/n
m — mass
mm — molar mass
n — moles of gas
(Gases) Ideal Gas Equation with Density
mm=(ρ/P)*RT
mm — molar mass P — pressure ρ — density R — Ideal Gas Constant (.0821) T — temperature (K)
(Gases) Density Equation
ρ=m/V
ρ — density
m — mass
V — volume
(Gases) Dalton’s Law of Partial Pressures
P=P₁+P₂+P₃+…
P — total pressure
Pₓ — partial pressure
