Gases and their Laws Flashcards
Everyday Gases:
1) Oxygen (O2)
2) Nitrogen (N2)
3) Helium (He)
4) Argon (Ar)
5) Carbon dioxide (CO2)
6) Acetylene (C2H2)
7) Propane (C3H8)
8) Butane (C4H10)
9) Nitrous oxide (N2O)
10) Freon (various chlorofluorocarbons)
1) medical use
2) fire suppression
3) balloons
4) provides an inert atmosphere for materials
5) carbonated soft drinks
6) welding
7) fuel for heat
8) fuel for lighters
9) anesthesia
10) refrigerators
Kinetic Theory of Gases:
1) Gases are…
2) The particles are…
3) The volume of the moles is…
4) When gas molecules collide,…
5) Electrical interaction…
6) The kinetic energy of gas molecules is…
1) composed of large numbers of particles.
2) in constant, random motion.
3) insignificant compared to the volume between the particles.
4) no kinetic energy is lost.
5) between particles is insignificant.
6) directly proportional to absolute temperature (Kelvin scale).
The rate of diffusion is…
inversely proportional to the mass of the molecule. Therefore, less massive molecules allow a quicker diffusion.
What is temperature?
It is a measure of the random motion of the molecules in a substance.
Since pressure is directly proportional to quantity, we can state…
the individual pressures add to the total pressure. (P1+P2+P3+…=PT)
The Gas Laws:
1) What is Boyle’s law?
2) What is Charle’s law?
3) What is Guy-Lussac’s law?
4) What is Avogadro’s law?
5) What is the ideal gas law?
1) Pressure is inversely proportional to volume. (P1V1=P2V2)
2) Volume is directly proportional to temperature. (V1/T1=V2/T2)
3) Pressure is directly proportional to temperature. (P1/T1=P2/T2)
4) Quantity is directly proportional to volume. (N1/V1=N2/V2)
5) PV=nRT or P1V1/n1T1=P2V2/n2T2
What are these individual pressures called?
Partial pressures
What is Dalton’s law?
It states the total pressure in a mixture of gases is equal to the sum of the partial pressures of the gases.
(P1/n1 = P2/n2 = P3/n3 = …PT/nT)
