Gas laws Flashcards

1
Q

Define total pressure

A

the total sum of all the collision forces

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2
Q

Define Charles’s law

A

For a fixed mass of gas at a constant pressure, the volume is directly proportional to the temperature

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3
Q

Name the four gas laws

A

-Charles’s law
-Boyles’s law
-Henry’s law
-Dalton’s law

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4
Q

Why is Charles’s law important?

A

Important in lung function testing as air cools as it is expired

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5
Q

Define Boyle’s law

A

For a fixed mass of gas the product of volume and pressure are always the same providing the temperature is constant.

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6
Q

What’s the equation for Boyle’s law?

A

P x V = constant

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7
Q

Using Boyle’s law what happens to volume when pressure increases?

A

volume decreases

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8
Q

Equation for Boyle’s law

A

P1 V1 = P2 V2

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9
Q

Using Boyle’s law what happens when you decrease volume?

A

-collisions increase
-presure increases

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10
Q

Draw the graph fo Charles’s law

A

straight line

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11
Q

Draw the graph for Boyles law

A

inversly proportional curve, look at powerpoint

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12
Q

Define atmospheric pressure

A

the constant movement and collision of gas particles exerts pressure

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13
Q

What is pressure exerted by air known as?

A

barometris pressure

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14
Q

what is barometric pressure measured in?

A

kilopascals (KPa)
or
mmHg

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15
Q

what is barometric pressure at sea level?

A

101KPa

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16
Q

What is 1KPa equal to in mmHg?

17
Q

What is 1mmHg equal to in Kpa?

18
Q

Example- if the barometric pressure is 760mmHg what is the Kpa?

A

760 x 0.133 = 101.1 KPa

19
Q

List the percentage of gases in the air

A

Nitrogen-78%
oxygen-20.8%
Argon-0.9%
Carbon dioxide-0.04%
other gases- 0.17%

20
Q

Define Dalton’s law of partial pressure

A

the total pressure of a mixture of gases is equal to the sum of the partial pressure that each gas would exert in isolation.

e.g 5KPa + 15Kpa = 20 KPa

21
Q

what is the equation for partial pressure?

A

% of gas x atmospheric pressure

22
Q

example- partial pressure of oxygen- 20.9%

A

20.9% x 101kpa
0.209 x 101KPa
=21.1 KPa

23
Q

at sea level the atmospheric pressure is 101KPa which is?

A

this is the sum of partial pressures of constitueant gases

24
Q

What are three factors that affect the movement of gases?

A

-pressure gradient
-solubility of gas in liquid
-temperature

25
define diffusion
the movement of a substance from an area of higher concentration to an area of lower concentration
26
The greater the partial pressure difference between the two areas....
more rapidly the gas moves
27
Define Henry's gas law
-gases dissolved in liquid -the number of molecules dissolving in liquid is directly proportional to the partial pressure at the surface of the gas
28
What is the equation for Henry's law and what does each part mean?
P = kH.C p-partial pressure of the gas in the atmosphere above the liquid C- concentration of dissolved gas KH-Henry's law constant of gas-depends on the solute, solvent and temperature
29
Give an example of what happens during Henry's law
-intital state-no O2 in solution -O2 dissolves -at equilibrium PO2 in air and water is equal. Low O2 solubility means concerntations are not equal
30
What happens to pressure at high altitudes?
decreases
31
What happens to the partial pressure of oxygen at a high altitude?
decreases
32
What is the KPa of oxygen at high altitudes of 33Kpa?
20.9% x 33 = 6.90KPa
33
Define water vapour pressure
the pressure exerted by molecules of water vapour in gaseous form
34
what is the water pressure vapour standard number?
PH20= 6.3KPa at 37 degrees body temp
35
what is the partial pressure of moist inspired oxygen?
PIO2 =20.9% x (PB - saturated water vapour pressure at 37 degrees pio2 = 0.209 x (101- 6.3) =0.29 x 94.7 =19.8
36
what are lung volumes measurements standardised and reported at?
body temperature and pressure saturated with water (BTPS)