Use mathematical software or an electronic spreadsheet to:Evaluate the change in entropy of 1.00 mol CO2(g) on expansion from 0.001 m3 to 0.010 m3 at 298 K, treated as a van der Waals gas.

(a) An ideal gas of mass 4.5 g and molar mass of 17 g.mole-1 occupies 12.7 L at 310 K. Answer the following questions based on the conditions presented. (i) Calculate the work done under a constant external pressure of 30 kPa until the volume of gas has increased by 3.3 L.  (ii) Calculate the work done in an isothermal and reversible expansion process resulting in a final volume of 16L. (iii)  If the gas has a molar heat capacity of 30.8 J.mol-1.K-1 and is subjected to a constant volume process until it reaches a temperature of 350K, calculate the heat transfer in kJ.mol-1 of the gas.       (b) Calculate the standard enthalpy of formation of N2O5 (g) from N2 (g) and O2 (g), in kJ. mol-1, from the following data:                                                                           2NO(g) + O2(g) ® 2NO2(g)      DH = -114.1 kJ   4NO2(g) + O2(g) ® 2N2O5(g)   DH = -110.2 kJ   N2(g) + O2(g)  ® 2NO(g)           DH = +180.5 kJ

Discuss the relations between: the entropy (particularly of the universe), the standard Gibbs' free energy change, the spontaneity, the equilibrium constant, and the equilibrium position for or associated with a process.

What is the chemical significance of a positive Gibbs free energy change and what is the chemical significance of an equilibrium constant significantly less than one?