3.6.2 Thermal Physics Flashcards

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1
Q

Define avogadro Constant

A

The number of atoms in 12g of carbon-12 (or the number of molecules in one mole of substance)

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2
Q

What does Boyle’s law state?

A

​The pressure of an ideal gas is inversely proportional to its volume when held at constant temperature.

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3
Q

What is brownian motion?

A

The ​random motion of larger particles in a fluid​ caused by ​collisions​ with surrounding particles (e.g. smoke and air)

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4
Q

What does Charles’ law state?

A

The volume of an ideal gas is directly proportional to its absolute temperature when held at constant pressure.

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5
Q

Define internal energy of a body

A

The sum of the randomly distributed kinetic energies and potential energies of the particles in a body.

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6
Q

What does the pressure law state?

A

​The pressure of an ideal gas is directly proportional to its absolute temperature, when the volume is fixed.

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7
Q

Define Specific Heat Capacity

A

The amount of energy required to increase the temperature of 1kg of a substance by 1 Kelvin without changing its state

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8
Q

Define Specific Latent Heat

A

The amount of energy required to change the state of 1kg of a substance without a change of temperature.

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9
Q

What are the energy changes during a state change?

A

the (mean/total) potential energy of the system is changing but the (mean/total) kinetic energy is not

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10
Q

2 ways to increase internal energy

A
  • Do work on the system to transfer energy to it
  • Heat (increase the temperature) of the system
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11
Q

How to observe Brownian motion

A

By looking at smoke particles under a microscope

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12
Q

What was Brownian motion used as evidence for?

A

Existence of atoms

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13
Q

5 assumptions for kinetic theory model

A
  • No intermolecular forces act on the molecules
  • Duration of collisions in negligibly in comparison to time between collisions
  • Collisions are perfectly elastic
  • Molecules move in straight lines between collisions
  • Size of gas molecules is negligible
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13
Q

How much potential energy does an ideal gas have?

A

None (as potential energy is associated with intermolecular forces)

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14
Q

Fundamental difference between gas laws and kinetic theory model?

A

The gas laws are empirical in nature whereas the kinetic theory model arises from theory

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15
Q

Boyle’s law explanation using kinetic theory model

A
  • If you ​increase the volume​ of a fixed mass of gas, its molecules will move further apart
  • so collisions will be less frequent
  • so force per unit area on surface on container decreases
  • therefore ​pressure decreases​
16
Q

Charle’s law explanation using kinetic theory model

A
  • When the ​temperature of a gas is increased​, the molecules mean kinetic energy increases
  • so the molecules mean speed increases
  • and because pressure is kept constant (therefore frequency of collisions is constant) the molecules ​move further apart and volume is increased​.
17
Q

Pressure law explanation using kinetic theory model

A
  • When the ​temperature of a gas is increased​, the mean kinetic energy of the particles increases
  • meaning their mean speed increases
  • as volume is constant, the frequency of collisions between molecules and their container increases and they collide at higher speeds
  • the rate of change of momentum (force exerted on container) increases
  • pressure is force / area
  • therefore pressure is increased​.
18
Q

Describe how the motion of the atoms changes when a gas’ temperature is increasing

A

The mean speed/kinetic energy increases

19
Q

Gas law interpretation of absolute zero

A

Temperature at which the volume/pressure of a gas extrapolates to zero

20
Q

Kinetic theory model interpretation of absolute zero

A

it is the temperature at which the kinetic energy of the particles can be extrapolated to be zero

21
Q

What do you talk about when using the kinetic theory to talk about P/V in/decreasing?

A

(Mean/Total) Momentum change!
Rate of collisions!

22
Q

What is meant by an ideal gas?

A
  • A gas that obeys the ideal gas laws at all temperatures and pressures
23
Q

What is represented by the area under a pressure volume graph?

A

The work done to the system

24
Q

Define the molar mass of a substance

A

The mass in grams of 1 mole of the substance

25
Q

How does the arrangement of the atoms change when changing from solid to liquid?

A
  • Some of the atomic bonds are broken
  • Allowing atoms to change from vibrating around fixed positions to being able to slide around each other
26
Q

Does the mark scheme refer to mean or average kinetic energy?

A

mean

27
Q

Define internal energy of an ideal gas

A

The sum of the randomly distributed kinetic energies of the particles in a gas.