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15) ideal gases Flashcards

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1
Q

What is Avagadro’s constant?

A

A number of particles equal to the number of atoms in 12 grams of carbon-12

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2
Q

What is one mole of a substance?

A

An amount in which the number of atoms/molecules is equal to Avogadro’s constant.

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3
Q

How do you find the mass of one atom from its nucleon number?

A

Multiply nucleon number by the atomic mass unit (u) in kg.

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4
Q

How is the atomic mass unit defined?

A

It is 1/12th the mass of a Carbon-12 atom

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5
Q

How do you calculate the number of particles from the number of moles of a substance?

A

Number of particles = number of moles × Avagadro’s constant

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6
Q

How do you find the molar mass of a substance from the molecular mass?

A

Molar mass = Molecular mass x Avagadro’s Number

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7
Q

How do you find the total mass of a substance from the number of moles?

A

number of moles x molar mass

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8
Q

How do you calculate the number of moles of a substance from the number of particles?

A

Number of particles÷Avagadro’s number

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9
Q

How do you find the molar mass of an element from its nucleon number?

A

Molar mass is equal to nucleon number in grams.

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10
Q

Boyle’s law: Pressure is inversely proportional to…

A

Volume for a fixed mass of gas at constant temperature

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11
Q

Charles’ law: Volume is proportional to…

A

Absolute temperature for a fixed mass of gas at constant pressure.

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12
Q

Gay Lassac’s Law: Pressure is proportional to…

A

Absolute temperature for a fixed mass of gas at constant volume

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13
Q

Avogadro’s law: Volume occupied by a gas is proportional to…

A

Number of particles/moles if pressure and temperature are constant.

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14
Q

How do you find absolute zero from a pressure temperature graph?

A

Extrapolate the line to find the x-intercept.

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15
Q

What is R in pV = nRT?

A

Molar Gas Constant (8.31)

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16
Q

What is N in pV = NkT?

A

Number of particles

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17
Q

What is n in pV = nRT?

A

Number of moles

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18
Q

What is k in pV = NkT?

A

Boltzmann constant

19
Q

What units of temperature should be used in the ideal gas equation?

A

Kelvin

20
Q

What is the equation of state for an ideal gas?

A

pV = NkT OR pV = nRT

21
Q

What is an ideal gas?

A

A theoretical gas that obeys the gas laws at all pressures and temperatures

22
Q

What are the SI units of pressure?

A

Pascal (Pa or Nm⁻²)

23
Q

What is the definition of pressure?

A

The force per unit area exerted normally to a surface

24
Q

What is the relationship between root mean square speed of particles in a gas and absolute temperature?

A

rms speed is proportional √(absolute temperature)

25
Q

Why does increasing the temperature of an ideal gas increase pressure?

A

Particles have greater kinetic energy so there is a greater rate of collisions and greater change in momentum per collision.

26
Q

Why does increasing the volume of an ideal gas decreases pressure?

A

P=F/A. Force exerted decreases as the rate of collisions with the container decreases and the surface area increases.

27
Q

According to Newton’s second law if a particle experiences a change in momentum…

A

There must be a force acting on the particle.

28
Q

According to Newton’s third law if a container exerts a force on a particle…

A

The particle must exert a force on the container.

29
Q

How do you calculate the mean square speed of gas particles from their velocity?

A

Square the magnitude of the velocity of each individual gas molecule and then take the average of these values.

30
Q

How do you calculate root mean square speed of a gas?

A

Square the magnitude of the velocity of each individual gas molecule, take the average of these values and then take the square root.

31
Q

Why is root mean square speed used instead of velocity?

A

Average velocity is zero.

32
Q

What is N in pV = ¹/₃ N m (c)²

A

Number of particles

33
Q

What is (c)² in pV = ¹/₃ N m (c)²

A

Mean square speed

34
Q

What is ³/₂kT equal to?

A

The mean kinetic energy of a gas particle

35
Q

What form is the internal energy of an ideal gas?

A

Purely kinetic (i.e. no potential energy)

36
Q

Why is there no potential energy in an ideal gas?

A

Because there are no force between particles (except during collisions).

37
Q

What is ³/₂NkT equal to?

A

Total internal energy of an ideal gas.

38
Q

Kinetic theory assumption concerning volume

A

The volume of the particles in a gas is negligible compared to the volume of the container

39
Q

Kinetic theory assumption concerning forces

A

There are no electrostatic forces between particles except during collisions

40
Q

Kinetic theory assumption concerning motion

A

Particles are in continuous, rapid, random motion.

41
Q

Kinetic theory assumption concerning collisions

A

The collisions particles undergo with each other and the container are all elastic

42
Q

Kinetic theory assumption concerning time

A

The duration of collisions is negligible compared to the time between collisions

43
Q

What is the relationship between absolute temperature and the average KE of particles in a substance?

A

Absolute temperature is proportional to average kinetic energy of the particles in a substance.

physics (18 decks)

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