The enthalpy of vaporization of ethanol is 38.56 kJ/mol. It has a boiling point of 351.44 K. What is the difference in entropy between ethanol's liquid and gaseous states at 351.44 K? What I'm asking is what is the size of the "jump" on the Sm versus Temperature curve.
Write out all equations (but you do not have to do the integration!) how you would calculate the absolute entropy of Cl2(g) at 298K. For full credit, you must include the limits of integration.