{Year 2} Chapter 4 - Thermal Physics (Up to page 74) Flashcards

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1
Q

What is the equation for internal energy?

A

U = Sum kinetic + sum potential, definition: ‘the sum of the randomly distributed kinetic and potential energies of the particles in a body’

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2
Q

What is the first law of thermodynamics?

A

The increase in internal energy of a system is equal to the heat added to the system minus the work done by the system, or deltaU = deltaQ - deltaW

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3
Q

What happens when a gas expands at a constant temperature?

A

It does work on its surroundings that can be calculated using the equation deltaW = pressure x deltaVolume

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4
Q

What is the letter for specific heat capacity and what is it?

A

c, specific heat capacity is the amount of energy is joules required to heat one kilogram of a substance one degree kelvin higher

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5
Q

What does the equation Q = ml mean?

A

Q is the amount of energy required to change a substance’s state without changing its temperature, m is mass, and l is specific latent heat

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6
Q

What is absolute zero?

A

The point at which no particles move, and thus there is no heat. Marked as 0 on the Kelvin scale, it is also equivalent to -273.15 degrees C. It is the lowest temperature possible

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7
Q

What is Boyle’s Law?

A

For a fixed mass of ideal gas at a constant temperature, the pressure of the gas is inversely proportional to its volume, aka p1 x v1 = p2 x v2

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8
Q

What is Amonton’s Law?

A

The pressure of a fixed mass and a fixed volume of gas is directly proportional to the absolute temperature of the gas

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9
Q

What are the three constants and their symbols?

A

Boltzman Constant (k), Avogadro’s Constant (N subscriptA) and the molar gas constant (R)

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10
Q

What is the main difference in how the gas laws and kinetic theory came to be recognised?

A

The gas laws were empirically found and based whereas kinetic theory is more theory based

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11
Q

What does the equation pV = nRT mean?

A

p = pressure, V = volume, n = moles, R = molar gas constant, NOT AVO’S CONSTANT, T = temperature

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12
Q

Name 3 assumptions made with an ideal gas.

A

Molecules are all identical, small, hard and spherical // Volume of the molecules is much less than that of the container // All the collisions between the particles are elastic and and all motion is frictionless // The molecules obey Newton’s Laws // The average distance between the molecules is much less than the size of them // They are constantly moving with Brownian motion (randomly) with a distribution of velocities around a mean // There are no attractive or opposing intermolecular forces other than when the particles collide // The time spent between collisions is much greater than the time spent colliding // there are no long range forces acting on the particles

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