The problem that I am trying to figure out is problem 3
2) The standard entropy of liquid methanol at 298.15 K is 126.8JK-1mo and its heat capacity is 81.6JK-mol. Methanol boils at 337.8 K with an enthalpy of vaporization at that temperature of 35.21 kJmol-. The heat capacity of the vapor is 43.89 JK-mol-1. Calculate the entropy of methanol vapor at 800 K. ) The heat capacity of solid silver in JK-mol- is given by the equation Cp.m = 2 1.2 + 4.27 x 10-3T + 1.51 x 105)T2 where T is the temperature in kelvins. What is the change in entropy per mole of silver when this substance is heated from 298 K (room temperature) to its melting point, 1234 K, at constant pressure? Compare this to the entropy change during the melting process. The heat of fusion for silver is 11.95 kJ mol-1 4) When a carbonate solution is acidified, carbon dioxide is produced.
