unit 12: gas laws Flashcards
boyles law
P1V1 = P2V2
Charles’ laws
V1/T1=V2/T2
Gay-Lussac’s law
P1/T1 = P2/T2
Avogadro’s law
V1/n1 = V2/n2
Combined gas laws
P1V1/T1 = P2V2/T2
Constant, non STP gas CONDITIONS (volume, temp, moles, etc.)
PV=nRT
Ideal gas constant for mmhg/torr
62.4 mmhg L / mol K
Ideal gas constant for atm
0.0821 atm L / mol K
Ideal gas constant for kPa
8.31 kPa L / mol K
Density calc at non STP
PM = DRT
Given grams, asks for volume at non stp
stoich, then PV=nRT
given liters, asks for mass at non stp
PV=nRT, then stoich
STP for mmhg/torr
760.0
STP for kPa
101.3 kPa
STP for psi
14.7 psi
STP for atm
1 atm, obviously
what relationship is boyles law and how does it work
gases are compressible, as volume decreases amount of collisions increase (particles closer together)
what relationship is charles law and how does it work
temp goes up, volume goes up because faster particles (higher temp) = more collisions and spreads out
what relationship is gay-lussacs law and how does it work
temp goes up, pressure goes up because faster particles means more collisions
how does avogadros law work
equal volumes of all gases, at
the same temperature and
pressure, have the same
number of particles
Ideal gas laws (5)
- particles move randomly and rapidly
- particles have no mass
- particles do not attract or repel each other
- particles are elastic (no energy gained or lost during collision)
- particles avg kinetic energy is exactly proportional to the temperature
what makes a gas more ideal? (5)
- little mass (like no mass)
- no electrons (less repel)
- Low pressure (further away particles, no repel)
- high temp (too fast, no repel)
- nonpolar or weak attractive forces (no repel)
