Thermal physics Flashcards

1
Q

Why do particles have random kinetic energies

A

They all have random speeds

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
2
Q

Why do particles have randomly distributed potential energies

A

Potential energy based on the particle’s relative positions to each other, which is random

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
3
Q

Define internal energy

A

Sum of the randomly distributed kinetic and potential energies of all the particles

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
4
Q

Which factor determines the speed and kinetic energy of particles

A

Temperature as it is a measure of the average kinetic energy of the particles in the system

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
5
Q

Define a closed system

A

No matter is transferred in and out so the internal energy is constant unless work is done

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
6
Q

How can you change the internal energy within a closed system

A
  • Increase by heating or doing work such as changing shape
  • Decrease by cooling

Since internal energy has changed, average KE and PE has also changed

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
7
Q

How does energy change during a change of state

A

Energy is going into breaking bonds and not increasing temperature so KE stays constant but PE rises and internal energy rises

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
8
Q

Define specific heat capacity

A

Energy required to raise temperature by 1°C or 1 K for a 1 Kg substance

Q = mcΔθ

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
9
Q

Define specific latent heat

A

Thermal energy required to change the state of a 1 Kg substance where l of vapourisation is for boiling and condensing and l of fusion is for melting or freezing

Q = ml

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
10
Q

What is absolute 0

A
  • Lowest temperature possible (0 K or -273 °C)
  • Means particles have minimum KE
How well did you know this?
1
Not at all
2
3
4
5
Perfectly
11
Q

Explain Boyle’s law

A

P ∝ 1/V at a constant T

Because decreased volume means particles are closer together so collide more with each other and container so exert more force on each other and container so more pressure

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
12
Q

How does a change in temperature affect the graph of pressure against volume

A
  • Normally looks like a graph of y = k/x
  • Increasing temperature causes shift out of the graph
  • A gas that obeys Boyle’s law at all temperatures is called an ideal gas
How well did you know this?
1
Not at all
2
3
4
5
Perfectly
13
Q

Explain Charles’ law

A

V ∝ T at a constant P

Because as T increases average KE is higher so speed increases meaning particles spread further apart from each other

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
14
Q

Describe the graph of V against T for an ideal gas

A

Straight line which passes through origin if in K or touches x axis at -273 if in °C (i.e. absolute 0)

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
15
Q

Explain The Pressure Law

A

P ∝ T at a constant V

Because as T increases average KE is higher so speed increases, meaning they collide and exert force on the walls more frequently with more force, meaning an increase in pressure

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
16
Q

Describe the graph of V against T for an ideal gas

A

Straight line which passes through origin if in K or touches x axis at -273 if in °C (i.e. absolute 0)

17
Q

What is the ideal gas equation

A

PV = nRT
or
PV = NkT

where N = n x 6.02x10^23
and k = R / (6.02x10^23)

18
Q

How can you calculate the work done in expanding or contracting a gas

A

Work done = P x ΔV

Area under a pressure volume graph

19
Q

What are the assumptions in the kinetic theory model

A

Remember VIRCE
- Volume of container is much larger than the volume of gas molecules
- Intermolecular forces between molecules are negligible
- Random motion of gas molecules
- Collision duration is negligible compared to the time between collisions
- Elastic collisions between gas molecules and container

20
Q

Derive PV = 1/3 Nm(crms)^2

A
  1. Change in momentum during collision = mu - (-mu) = 2mu
  2. Time between collisions = 2l/u
  3. F = 2mu /(2l/u) = mu^2 /l
  4. P = (mu^2 / l) / (l^2) = (mu^2) / l^3 = mu^2 / V
  5. For N particles, x by N and use the average speed (rms to ignore (-)s)
    so P = Nm(urms)^2 /V
  6. u is only 1 of 3 directions which make up resultant velocity c so urms^2 = 1/3 crms^2 (with Pythagoras)
    P = (Nm (crms^2 / 3)) / V
    so PV = 1/3 Nm crms^2
21
Q

Derive the average kinetic energy equation u

A
  1. nRT = 1/3 Nm crms^2
  2. (x 3/2) so
    3/2 nRT = 1/2 Nmcrms^2
  3. 3/2 NkT = 1/2 Nm crms^2
  4. 3/2 kT = 1/2 m crms^2
    and 1/2 m crms^2 is the average KE of 1 molecule
22
Q

Explain Brownian motion

A

Where large particles in a fluid collide with the small fast moving fluid particles, causing random zig-zag motion i.e. Brownian motion

23
Q

How does Brownian motion help prove the kinetic theory

A

Kinetic theory assumes that particles have random motion so assumption would be wrong if not for Brownian motion