Chapter 12- Gas Laws And Kinetic Theory Flashcards

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1
Q

Pressure eq

A

Pressure = force/ area

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2
Q

Pressure unit

A

N/m^2 = Pa

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3
Q

Pascal definition

A

A pascal is the pressure exerted by a force of 1N acting at right angles to an area of 1m^2

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4
Q

A fluid is a substance that can

A

Flow

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5
Q

Both liquids and gases are

A

Fluids

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6
Q

Pressure density eq

A

Pressure= density x g x 🔺h

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7
Q

Pressure on base eq

A

Weight of column of water / area

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8
Q

Don’t forget to add on the pressure of the _____ in questions

A

Pressure of the atmosphere

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9
Q

If a liquid is stationary then the pressure must act

A

Equally in all directions

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10
Q

Boyle’s law

A

The pressure of a fixed mass of gas is inversely proportional to the volume, provided the temperature is constant

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11
Q

Boyle’s law equations

A

P~ 1/V

P1V1 = P2V2
If T1=T2

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12
Q

Isothermal def

A

The same temperature

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13
Q

Charles’ law

A

The volume of a fixed mass of gas is directly proportional to its absolute temperature provided the pressure is constant

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14
Q

Charles’ law eq

A

V~T

V1/T1 = V2/T2
Providing P1=P2

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15
Q

Pressure law

A

The pressure of a fixed mass of gas is directly proportional to its absolute temperature provided the volume is constant

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16
Q

Pressure law eq

A

P~T

P1/T1= P2/T2

(V1=V2)

17
Q

Ideal gas equation

A

pV = nRT

18
Q

What is R in the ideal gas equation

A

R= molar gas constant

= 8.31 Jmol^-1K^-1

19
Q

Alternative ideal gas equation

A

pV = NkT

20
Q

What is k in the alternate ideal gas equation.

A

k= Boltzmann constant

= 1.38x10^-23 JK^-1

21
Q

Avogadro’s hypothesis

A

1 mole of gas should always occupy the same volume for a given temperature and pressure

22
Q

What is standard temperature

A

298 K

25*C

23
Q

What is standard pressure

A

101 kPa

24
Q

Brownian motion

A

Random jerky motion of particles suspended in a fluid resulting from their bombardment by molecules in the fluid

25
Q

Examples of Brownian motion

A
  • pollen on water
  • soot particles in a smoke cell
  • bromine gas diffusion
26
Q

6 assumptions for kinetic theory of gases

A

1) gas consists of v large number of molecules
2) move with continuous, rapid, random motion
3) collisions are always perfectly elastic
4) volume occupied by molecules is negligible compared with volume of container
5) intermolecular forces are negligible except during a collision
6) duration of collisions is negligible compared with time spent in between collisions

27
Q

Kinetic model explains…

A

The macroscopic properties of a gas in terms of the microscopic motion of the particles

28
Q

What kind of motion are gas molecules in a container

A

Continuous
Rapid
Random motion

29
Q

How is pressure created for kinetic model of gas in container

A

Gas molecules moving in container
Colliding with wall of container
Change in momentum of molecule after elastic collision
Molecules exert a force per unit area on the wall
This force per unit area is pressure

30
Q

Average force equation for the molecule colliding with wall over a time period

A

= mvx^2 / length

x= velocity in x direction 
l= length of the side of the cube
31
Q

If there are N molecules moving with velocities vx, vx2, vx3
What is eq for the mean square speed of these velocities

A

= vx^2 + vx2^2 + vx3^2 / N

32
Q

N molecules what is average force eq

A

= Nm/l (Vx^2)

33
Q

What is the eq involving density and pressure

A

p= 1/3 ‘rho’

34
Q

Mean kinetic energy eq for kinetic theory of temperature

A

Mean KE= 3/2 kT

All have some molecular KE at given temp
Mean KE is zero at absolute zero
More massive molecules are moving more slowly