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Chem 120 > Chapter 4 - Ideal Gas Laws > Flashcards

Chapter 4 - Ideal Gas Laws Flashcards

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1
Q

what are phases and phase transitions?

A

there are just three states of matter

  1. solid
  2. liquid
  3. gas
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2
Q

what does fusion mean?

A

melting

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3
Q

what does vaporization mean?

A

aka boiling

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4
Q

what does crystallization mean?

A

freezing

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5
Q

what does condensation mean?

A

conversion of vapour gas into liquid gas

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6
Q

what is the kinetic molecular theory?

A

it describes the behaviour of gases

  1. Gas molecules are extremely small (mass but no volume)
  2. Gas is in constant, random, straight-line motion, collisions are elastic
  3. Molecules of gas experience no intermolecular forces
  4. Gas molecules span a distribution of speeds, and average kinetic energy is directly proportional to temperature
  5. Ideal gases satisfy all these criteria under most ordinary conditions
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7
Q

do ideal gases experience phase changes?

A

no phase changes with ideal gases because by definition there are no intermolecular forces

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8
Q

what is barometric pressure?

A
  • used to measure atmospheric pressure
  • uses mercury (high density, p=13.5951g/ml at 0degrees)
  • the atmosphere exerts the same pressure on the surface of the mercury both inside and outside the tube, and the liquid levels are equal
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9
Q

comparing liquid pressures?

A 
use this formula to compare liquid pressures 
P = hgd
h - height of column
g - gravity (9.81)
d - density
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10
Q

what are manometers?

A

pressure gauge for determining the pressure of a gas

  1. Patm > Pgas; Pgas = Patm - ΔH
  2. Patm
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11
Q

What is the ideal gas law?

A

relationship between volume, temperature and pressure of and ideal gas

PV = nRT

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12
Q

what is R when pressure units are in bars?

A

R = 0.083145

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13
Q

what is R when pressure units are in atmospheres?

A

R = 0.08206

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14
Q

What is R when pressure units are in Joules?

A

R = 8.3145

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15
Q

what is the general gas equation?

A

sometimes a gas is described under two different conditions, initial (1) and final (2)
P1V1/n1T1 = P2V2/n2T2

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16
Q

what is Charles law?

A

Charles law states that volume and temperature are directly proportional at constant pressure

V1/T1 = V2/T2

17
Q

What is Boyle’s Law?

A

Boyle’s law states that pressure is inversely proportional to volume at constant pressure

P1V1 = P2V2

18
Q

What is Amonton’s law?

A

Amonton’s law states that pressure is directly proportional to temperature at a constant volume

P1/T1 = P2/T2

19
Q

what is Avagadro’s Law?

A

Avagadro’s law states that the volume of gas is directly proportional to the amount of gas at a fixed temperature and pressure

V1/n1 = V2/n2

At STP 1mol of gas equals 22.7L of gas

20
Q

what is the Molar mass determination from the ideal gas law?

A

M = mRT/PV

21
Q

what is the density determination from the ideal gas law?

A

d = MP/RT

22
Q

The density of a gas is…?

A

The density of a gas is proportional to its molar mass: the lower the molar mass, the greater its lifting power

23
Q

what is a mixture of gases?

A
  • Partial pressure is the pressure that molecules of each gas exert
24
Q

What is Dalton’s Law of Partial Pressure?

A

it states that the total pressure of mixture of the gases is the sum of the partial pressures of each of the individual gases that make up the mixture

Ptotal = Pa + Pb +....
Pa = Xa * Ptotal
25
Q

What is mole fraction?

A 
Xa = n(a)/n(total) = Pa/Ptotal = Va/Vtotal
n(total) = n(a) + n(b) +...
Ptotal = Pa + Pb +....
Vtotal = Va + Vb +....
26
Q

what is Root Mean Square Velocity (Urms)?

A
  • Close to the average speed of the particle
  • Inversely proportional to the molecular mass of the gas
  • molecular mass in kilograms (kg)
  • R = 8.3145 J/mol*K
  • M = molar mass

Urms = ✓3RT/M

27
Q

What is the Ideal vs Non-ideal gas?

A

Van der Waaals Equation: RT = (P + a/Vm^2)(Vm - b); Vm = molar volume

  • Real gas must include the volume of the gas particles
  • Real gas has intermolecular forces unlike ideal gases
28
Q

When do real gases behave Ideally?

A

Gases behave ideally at..

  1. High temperatures
  2. Low Pressures
29
Q

In Van der Waals Equation what do (a) and (b) do?

A

(a) - larger (a) means stronger attraction and lower pressure
(b) - larger (b) means more excluded volumes and higher pressure

30
Q

Directly proportional means?

A

If variables are on the opposite side of each other in an equation or they’re divided by each other, they are directly proportional to each other
(Eg. if one increase the other increase)

31
Q

Inversely proportional means?

A

If variables are on the same sides of the equation as each other, or if they are multiplied by each other they are inversely proportional
(Eg. If one increase the other decrease)

Chem 120 (3 decks)

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