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15. Ideal gases

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  1. 15.1 The mole

    1. • understand that amount of substance is an SI base quantity with the base unit mol

    2. • use molar quantities where one mole of any substance is the amount containing a number of particles of that substance equal to the Avogadro constant NA

  2. 15.2 Equation of state

    1. • understand that a gas obeying pV ∝ T, where T is the thermodynamic temperature, is known as an ideal gas

    2. • recall and use the equation of state for an ideal gas expressed as pV = nRT, where n = amount of substance (number of moles) and as pV = NkT, where N = number of molecules

    3. • recall that the Boltzmann constant k is given by k = R / NA

  3. 15.3 Kinetic theory of gases

    1. 15.3.1The basic assumptions of the kinetic theory of gases

      • state the basic assumptions of the kinetic theory of gases

    2. 15.3.2How molecular movement causes the pressure exerted by a gas and derive and

      • explain how molecular movement causes the pressure exerted by a gas and derive and use the relationship pV = 1/3 Nm<c2> • Where <c2> is the mean-square speed (a simple model considering one-dimensional collisions and then extending to three dimensions using 1/3 <c2> = <cx 2> is sufficient)

    3. 15.3.3The root-mean-square speed cr.m.s. is given by c<>2

      • understand that the root-mean-square speed cr.m.s. is given by c<>2

    4. 15.3.4PV = 1/3 Nm<c2> with pV = NkT to deduce that the average translational

      • compare pV = 1/3 Nm<c2> with pV = NkT to deduce that the average translational kinetic energy of a molecule is 3/2 kT, and recall and use this expression