15 : Ideal gases Flashcards

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1
Q

Define a mole

A
  • The amount of substance that contains as many elementary entities as there are atoms in 0.012kg of carbon-12
  • this is avogadro constant
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2
Q

Total number of molecules in a substance equation

A

N = n x Na
Total number of molecules in a substance = number of moles of the substance x avogadro constant

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3
Q

amount of matter equation

A

m = n x M
Amount of matter = molar mass x number of moles

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4
Q

Assumptions

A
  • very large number of molecules moving in random directions at random speeds
  • occupy negligible volume compared to volume of container
  • collisions are perfectly elastic
  • electrostatic forces are negligible apart from during collisions
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5
Q

total change in momentum

A

when a single atom collides with container wall elastically peed does not change goes from +mu to -mu so total change is -2mu

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6
Q

pressure and volume

A
  • temperature and mass remain constant
  • pressure is inversely proportional to volume
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7
Q

pressure and temperature

A
  • volume and mass remain constant
  • pressure is directly proportional to temerpature
  • T in kelvin
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8
Q

estimating absolute zero

A
  • extrapolate p/T graph x-axis intercept is absolute zero
  • T in celsius
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9
Q

Maxwell-Boltzmann distribution

A
  • at any temperature the random motion and collision of particles means some are travelling very fast whilst others are barely moving.
  • the range of speeds at a given temp is the distribution
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10
Q

temperature and distribution

A

Changing temperature of the gas changes the distribution. the hotter the gas the greater range of speeds. the modal speed nd the r.m.s speed increase and the distribution becomes more spread out

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11
Q

Boltzmann constant

A

molar gas constant divided by avogadro constant

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12
Q

particle speeds at same temperatures

A
  • at a given temperature the molecules of different gases have the same average kinetic energy
  • the molecules have different masses
  • higher masses = smaller speeds
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13
Q

why is helium not in earth’s atmosphere

A
  • small mass and therefore high speed
  • when molecule has a greater speed than the r.m.s speed
  • higher speed then escape velocity of 11kms-1 so can escape earths atmosphere
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14
Q

internal energy of an ideal gas

A
  • sum of kinetic and potential energies
  • assumption - electrostatic forces are negligible except during collisions.
  • thus no electrical potential energy in an ideal gas
  • internal energy is just kinetic energy
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15
Q

Temp increases, oven isn’t sealed show that internal energy stays the same

A
  • The atmospheric pressure of the oven is constant at 1E5
  • since p=F/A force exerted on the walls which is equal to rate of change in momentum
  • higher oven temperature means higher average kinetic energy leading to more frequent collisions with greater momentum leading to a greater force
  • number of molecules in oven must decrease to keep pressure constant
  • pV=NkT thus T = (Pv)/(Nk)
  • total internal energy is given by 3NkT/2 thus T=2E/(3Nk)
  • rearrange E=3pV/2
  • showing that the internal energy E depends on pressure and volume only and therefore is independent of temperature.
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16
Q

Newtons law and pressure

A
  • free to move with constant random motion wih no forces of attraction = 1st law move with constant velocity
  • particles collide with the walls it exerts a force on the wall = newtons 3rd law wall exerts an eual and opposite force on particle
  • size of force = 2nd law f=rate of change in momentum = 2mu
  • significant number of particles all colliding at any given moment