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a van der Waals equation of state for 1 mole of a real gas is (p+ 2) (v – b) = RT V2 a + . Sketch the variation of p with V that this equation predicts at a temperature below the critical temperature, . Sketch the actual variation of p with V for Argon at a temperature below its critical temperature, clearly marking the range of volumes over which the Argon will exist as a liquid, a vapour and as a mixture of liquid and vapour. . For Argon b = 6.7 x 10-6 m' mol-l. Provide with justification an equation that relates b to the volume of a molecule and hence calculate the radius of an Argon atom. Describe what you would observe if 1 mole of Argon contained in a vessel with a volume equal to the critical volume is heated from a temperature below the critical temperature to a temperature above the critical temperature,