a) Calculate the change in entropy (deltaS) when one mole of diamond is heated from a temperature of 0 K to 400 K at a constant pressure of 1 bar. The temperature-dependent heat capacity of diamond is Cv ? 2.9x10-7 T3 J/(mol K), where T is the absolute temperature in K. b) Given that the entropy of diamond is zero at 0 K, calculate its absolute molar entropy at 400 K from the above result.