Gas Laws Flashcards
Postulate 1 of the Kinetic Molecular Theory
Gases are tiny particles, far apart relative to their size.
Postulate Two of Kinetic Molecular Theory
Gas particles are in continuous, rapid, random motion.
Postulate Three of the Kinetic Molecular Theory
No attractive forces between molecules under normal conditions of pressure and temperature.
Postulate Four of the Kinetic Molecular Theory
Collisions between gas particles and container walls are elastic.
Postulate Five of the Kinetic Molecular Theory
Temperature of a gas depends on the average kinetic energy (K=1/2mv^2).
Describe the relationship between pressure and volume.
Inversely related. Negative slope on a graph.
Describe the relationship between pressure and temperature.
Directly proportional. Positive slope on a graph.
Describe the relationship between volume and temperature.
Directly proportional. Positive slope on a graph.
Boyle’s Law
P1V1 = P2V2
Charles’ Law
V1T2 = V2T1
Gay-Lussac’s Law
P1T2 = P2T1
Combined Gas Law
P1V1T2 = P2V2T1
Temperature at STP
0°C, 273 K
Pressure at STP
1 atm, 101.32 kPa
Avogadro’s Principle: Equal _____ of gases contain equal _____
Avogadro’s Principle: Equal volumes of gases contain equal numbers of moles
Ideal Gas Law
PV = nRT
Universal Gas Constant (R)
0.0821 atm(L)/mol(K) or 8.314 kPa(L)/mol(K)
Dalton’s Law of Partial Pressure
The total pressure of a mixture of gases equals the sum of the partial pressures of the individual gases. Ptotal = P1 + P2 + …
Diffusion
Spreading of gas molecules throughout a container until evenly distributed.
Effusion
Passing of gas molecules through a tiny opening in a container.
Graham’s Law of Diffusion/Effusion
Smaller mass results in a higher rate of effusion. Nearly identical masses have nearly identical rates of effusion.
What is the conversion factor for kPa to atm?
101.32 kPa = 1 atm
