Section 6 part 3 - gases Flashcards

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1
Q

What is the pressure of a gas?

A

Force per unit area that the gas exerts normally

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2
Q

What does the pressure of a gas depend on?

A

Temperature, volume of container, mass of gas in container

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3
Q

What is an isothermal change?

A

Any change at constant temperature

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4
Q

Define Boyle’s law

A

For a fixed mass of gas at constant temperature, the gas pressure multiplied by the volume of gas is a constant

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5
Q

What graph would you plot when investigating Boyle’s law to get a straight line graph?

A

Pressure against 1/Volume, as p/1/V = pV, representing y=mx, where y is pressure, gradient is constant, and x is 1/volume

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6
Q

What type of graph do you get for Boyle’s law when plotting pressure against volume?

A

Reciprocal looking curves, with higher temperatures shifting the curve to the right, or with p against 1/v, a steeper gradient for higher temps

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7
Q

Define Charles’ law

A

For an ideal gas at constant pressure, the volume divided by the temperature is a constant

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8
Q

What is an isobaric change?

A

Any change at constant pressure

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9
Q

What is the work done by a gas on a piston equal to when changing the volume of the gas?

A

Pressure x change in volume

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10
Q

Define the pressure law

A

For an ideal gas with a constant volume, the pressure divided by the temperature is a constant

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11
Q

What causes the pressure of a gas on a surface?

A

The gas molecules hitting the surface

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12
Q

What is Brownian motion?

A

The random motion particles travel, due to the individual molecules bombarding each particle unevenly and randomly

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13
Q

How did Robert Brown show the existence of molecules and atoms

A

With pollen grains in the water`

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14
Q

What happens to the Brownian motion when temperature is increased?

A

The motion gets more erratic, but stays random

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15
Q

How much greater is the density of oxygen than that of hydrogen at constant temperature?

A

x16

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16
Q

Define the Avogadro constant

A

The number of atoms in 12g of the carbon isotope of 12/6C . = 6.02e23

17
Q

What is an atomic mass unit?

A

1/12th of the mass of a 12/6 Carbon atom.

18
Q

What is molarity?

A

The number of moles in a given quantity of a substance. Unit mol

19
Q

What is molar mass?

A

The mass of 1 mol of the substance, unit kg/mol

20
Q

What does the number of moles in mass Ms of a substance equal?

A

Mass of the substance (Ms) / the molar mass

21
Q

What does the number of molecules in mass Ms of a substance equal?

A

Avogadro’s constant (Na) x mass of the substance (Ms)/ molar mass

22
Q

What is a mole?

A

One mole of a substance consisting of identical particles is defined as the quantity of substance that contains Na particles

23
Q

What is an ideal gas?

A

A gas that obeys Boyle’s law

24
Q

What is the equation for an ideal gas?

A

pV/T = constant for a fixed mass of ideal gas

25
Q

What assumptions does the ideal gas equation make?

A

The pressure, volume and temperature of a fixed mass of gas all change

26
Q

what is R in the equation pV=nRT?

A

Molar gas constant, 8.31 J/mol kelvin

27
Q

What are the other equations for density of an ideal gas?

A

density = mass/volume = number of moles x molar mass of substance / volume. pressure x molar mass of substance/ R x temperature

28
Q

What are the other equations for the density of an ideal gas (not worded)

A

density = nM/V, pM/RT

29
Q

For an ideal gas at constant pressure, what is the relationship between density and the temperature?

A

The density is inversely proportional to the temperature

30
Q

State what each component of the equation pV=nRT is

A
p = pressure
V = volume
n = number of moles
R = molar gas constant, 8.31
T = Temperature
31
Q

State what each component of the equation pV=NkT is

A
p = pressure
V = volume
N = number of molecules
k = Boltzmann constant, R/Na, 1.38e-23
T = temperature
32
Q

How do you convert from Celsius to Kelvin?

A

Celsius + 273

33
Q

What happens to the root mean square when the temperature of the gas is raised?

A

The molecules move faster on average, so the rms increases

34
Q

What happens to the distribution curve of the rms when the overall rms increases?

A

The curve becomes flatter and broader because there are more molecules moving at higher speeds

35
Q

Briefly summarise the 5 assumptions made in the kinetic theory

A
  1. Molecules are point molecules
  2. Molecules do not attract each other
  3. Molecules move in continual random motion
  4. Collisions with the surface are elastic collisions
  5. Each collision with the container surface is of much shorter duration than the time between impacts
36
Q

KE Theory assumption: Why do you assume the molecules are point molecules?

A

So the volume of each molecule is negligible when compared with the volume of the gas

37
Q

KE Theory assumption: Why do you assume the particles do not attract each other?

A

If they did attract each other, the effect would be to reduce the force of their impacts on the container surface

38
Q

KE Theory assumption: Why do you assume the collisions with each particle and the container surface are elastic

A

So there is no overall loss of kinetic energy in the collision

39
Q

For an ideal gas, what is its internal energy given by?

A

The kinetic energy of the molecules in the gas