One mole of chlorine undergoes adiabatic reversible expansion from 1 dm^3 to 10 dm^3 with initial temperature of 273 K. Calculate q, w, AU and AH if the gas is considered a van der Waals gas. Given: a = 655 dm^3 kPa mol^2, b = 0.055 dm^3 mol¹. Cr, m = 33.91 J K¹ mol¹. Since the gas undergoes adiabatic reversible expansion,

4. The heat capacity of solid lead oxide is given by the equation: Cp(T) = 44.35 + 1.47 × 10-3 xT with T in units of K and the resulting Cp(T) in units of K-mol Calculate the change in enthalpy of 1 mole of PbO(s) if it is heated from 200 to 600 K at constant pressure. (Assume no phase transitions take place during this process.)

Recall that the van der Waals equation of state—an extension of the ideal gas equation—attempts to better capture the behavior of real gases. It can be written to parallel the PV = nRT form of the ideal gas equation:                                (P + an2/V2) (V − nb) = nRTa) For one mole of a van der Waals gas, derive an expression for the work done by a reversible and isothermal change in volume. In other words, evaluate the following integral for the van der Waals gasw = − {integral with limits from v1 to v2}  PdV.b) What are physical interpretations of the van der Waals constants a and b?c) If for helium, the van der Waals constant b is equal to 2.43 × 10–5m3 mol-1, using this value for b, calculate the diameter of the helium atom.

A sample consisting of 2.0 mol CO2 occupies a fixed volume of 15.0 dm3 at 300 K. When it is supplied with 2.35 kJ of energy as heat its temperature increases to 341 K. Assume that CO2 is described by the van der Waals equation of state, and calculate w, ∆U, and ∆H.