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FRCA Physics > Basic Units + Gas Laws > Flashcards

Basic Units + Gas Laws Flashcards

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1
Q

Equal values of
1 atmosphere

In Bar

A

1.01

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2
Q

1 atmosphere = ?PSI

A

14.69

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3
Q

1 atmosphere = ?kPa

A

100 (101.3)

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4
Q

1 atmosphere = ?mmHg

A

760

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5
Q

1 atmosphere = ?cm H2O

A

1020

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6
Q

1 atmosphere = ?Pascal

A

101, 325

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7
Q

How is SI unit for seconds standardised?

A

It is the duration for a certain number of oscillations of caesium-133 atom.

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8
Q

How are the SI units for meter standardised?

A

Length light travels in vacuum in 1/300000000 of a second.

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9
Q

How is mole standardised to?

A

Amount of substance that contains same number of particles as there are atoms in 0.012kg (12g) of carbon-12

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10
Q

Regarding derived and non-SI units:
1. Derived units must always be expressed as base units? T/F

  1. Velocity and speed have the same bad units? T/F
A
  1. False, can be expressed as base units or combination

2. True

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11
Q

What is the formula for kinetic energy?

A

1/2 mass x velocity squared

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12
Q

Force formula

A

Mass x Acceleration

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13
Q

Define pressure

A

Pressure is defined as the cumulative force generated, divided by the total area over which that force is applied.

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14
Q

What is Boyles Law?

A

At a constant temperature, the volume of a gas at a given mass will decrease if it’s pressure is increased.

Volume of a given mass of gas varies inversely with absolute pressure.

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15
Q

What is Charles Law?

A

At a constant pressure,
the volume of of a given mass varies with the absolute temperature.

Volume inversely proportional to Temp (Kelvin)

(Ie as temperature rises, gas moves more and hits sides of container therefore pressure would increase. To keep pressure constant volume of gas would have to increase to compensate.)

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16
Q

What is Gay-Lussacs Law?

A

At a constant volume, the absolute pressure of a given mass varies with absolute temperature.

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17
Q

What is the Kinetic Theory of gases?

What are the 4 postulates of Kinetic Theory?

A
  • is a model of gas behaviour that describes an imaginary, ideal gas.
    1. Gases contain a large number of particles.
    2. Individual particles are moving in random directions at random speeds.
    3. Individual particles travel in a straight line.
    4. There are no attractive or repulsive forces between particles.
18
Q

What is Brownian Motion?

A

Provides a demonstration that fluids are really made up of fast moving particles.

19
Q

What does the Maxwell-Boltzmann curve describe?

A

At a given temperature, a gas of a higher molecular weight has particles moving at a lower average speed. Hence, the distribution of the curve shifts to the left.

20
Q

Is the speed of gas particles directly proportional to kinetic energy and why?

A

No because kinetic energy varies with the square of the speed is governed by the equation:

  • kinetic energy = 1/2mv(squared)
21
Q

How does temperature effect the speed of a gas on a distribution curve and why?

A

Shifts to the right as speed increases with temperature.

22
Q

How would you describe temperature in relation to particles of gas?

A

Temperature is a reflection of the average kinetic energy of the particles of a gas.

23
Q

Graham’s Law?

A

Rate of diffusion of a gas is inversely proportional to the square root of its molecular weight.

24
Q

What is the combined gas law?

A

(Pressure x volume) / Temp = constant

Combination of three laws. Temp must always be in Kelvin but other units can be used for pressure and volume.

25
Q

What is Avogadro Principle?

A

States that equal volumes of all gases, at the same temp and pressure, must have the same number of molecules.

Hence the measurement of mole- number of particles.

26
Q

What is a mole?

A

A quantity of a substance containing the same number of particles as there are atoms in 12g of carbon 12.

This is equal to 6.022 x 10’23rd

27
Q

What is the value of R, the universal gas constant?

A

8.31 J K-1 mol-1

28
Q

What is the Ideal Gas Law

A

It combines Avogadro’s number and ideal gas law.

PV/T = C
Where C is the constant which is proportional to the amount of gas, n, which is Avogadros Law.

The proportionality factor is the universal gas constant R therefore:

C = nR

29
Q

What does Daltons Law of Partial Pressure state?

A

In a mixture of gases the pressure exerted by each gas is the same as that which it would exert if it alone occupied the container.

PT = (n1 + n2…)RT

30
Q

What is critical temperature?

A

The temperature above which a substance cannot be liquefied however much pressure is applied.

31
Q

What is the critical temperature of oxygen?

Nitrous oxide?

A

Oxygen: -119 degrees C

Nitrous Oxide: 36.5 degrees C

32
Q

What is critical pressure?

A

Critical pressure is the saturated vapour pressure of a substance at its critical temperature.

33
Q

Regarding the behaviour a gas:

  1. When does behaviour deviate from an ideal gas?
  2. What is the weight of one mole of nitrous oxide and what volume would it occupy at STP?
  3. What is the equivalent mass of one mole of oxygen and what volume would it occupy at STP?
A
  1. When temperature falls and pressure rises
  2. 44g is one mole, occupies 22.4L
  3. 32g is one mole, occupies 22.4L
34
Q

Would one mole of oxygen at 1 atmosphere pressure and room temperature occupy 22.4L?

A

No because the rule is that one mole would occupy this volume at standard temperature - 273.15 Kelvin - not room temperature.

35
Q

True/False

Regarding the ideal gas law
PV = nRT

  1. n must always be great than 1
  2. Temperature must always be expressed in Kelvin
  3. Measurements must always be taken at standard pressure and temperature
  4. The unit of ideal gas is in moles
A
  1. False, must be greater than or equal to zero.
  2. True
  3. False, hence the P and T in the equation as variables.
  4. False, it is J K mol
36
Q

What is saturated vapour pressure?

A

It is the partial pressure exerted by the vapour which is in equilibrium with its liquid.

37
Q

What is Henry’s Law?

A

At a fixed temperature - the amount of a given gas dissolved in a given liquid is directly proportional to the partial pressure of the gas in equilibrium with the liquid.

38
Q

What are the Bunsen and Otswald solubility coefficients?

A

Two ways of describing how gases are dissolved in solution.

Bunsen- the volume of gas corrected to STP and dissolved in a unit volume of a liquid at the temperature concerned where the patty oak pressure of the gas above the liquid is one atmosphere.

Otswald- the volume of gas dissolved in a unit volume of liquid at temperature concerned.

Otswald preferred by anaesthetists as it is not corrected to STP.

39
Q

How does knowledge of gases in solution explain why giving a patient fracture ribs and pneumothorax Entonox (nitrous oxide in oxygen) be risky?

A

The pneumothorax contains nitrogen and gas lower solubility than nitrous oxide, therefore nitrous oxide diffuses into the closed cavity faster than nitrogen diffuses out.

This would increase pneumothorax volume.

40
Q

Define density

A

Mass per unit volume

P = kg/m’3

41
Q

How is the specific density of gas measured?

A

Relative to air.

Specific density > 1 = more dense than air.

< 1 = less dense than air.

Liquids and solids are given relative densities to water.

42
Q

What is viscosity and what is it’s units?

A

Viscosity of the tendency of a fluid to resist flow, “fluid friction”, measured in Poise(P).

FRCA Physics (16 decks)

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