Gases

Question 1

What are the diatomic gases?

Answer 1

Hydrogen, Nitrogen, Fluorine, Oxygen, Iodine, Chlorine, & Bromine

Have No Fear Of Ice CoLd BeeR

Question 2

What is the formula for pressure?

Answer 2

P=F/a
Pressure = force/area

Question 3

What is Boyle’s Law?

Answer 3

P1V1=P2V2

Pressure (atm) and Volume (L) are inversely proportionaly under constant temperature and moles

Question 4

What is Charles’s Law?

Answer 4

V1/T1=V2/T2

Volume (L) and temperature (K) are directly proportional under constant pressure and moles

Question 5

What is Avogadro’s Law?

Answer 5

V1/n1=V2/n2

Volume (L) and Moles (mol) are directly proportional under constant pressure and temperature.

Question 6

What is Gay-Lussac’s Law?

Answer 6

P1/T1=P2/T2

Pressure (atm) and temperature (K) are directly proportional under constant volume and moles.

Question 7

What is the Combined Gas Law?

Answer 7

P1V1/n1T1=P2V2/n2T2

The ratio of initial pressure (atm) and volume (L) to temperature (K) and moles (mol) to its final state

Question 8

What is the ideal gas law?

Answer 8

PV=nRT
R = 0.0821 (atm)
or R = 8.314 (kPa)

Ideal at lower pressure and high temperature
STP - standard temperature and pressure is 1atm and 273K

Question 9

What are the 5 postulates of the Kinetic-Molecular Theory of Gases?

Answer 9

1. Particles are in constant, random motion
2. Combined volume of particles is negligible
3. Particles exert no forces on one another
4. Gas molecule collisions are elastic (no IMF)
5. All gases have same average kinectic energy at a given temp.

Question 10

What is Dalton’s Law of Partial Pressure?

Answer 10

Ptotal = P1 + P2 + ….
P1 = X1Ptotal (X1 is mole fraction of gas 1)

Total pressure of mixture is equal to the sum of partial pressures of individual gases

Question 11

What is gas density?

Answer 11

d = PM/RT
M = molar mass
T (in K)