 Please Visit Our Sponsors
 10.6 Absolute Entropies The entropy of a substance increases as the temperature is increased. This is readily understood because the addition of heat to a substance results in an increase in molecular randomness. Conversely cooling a substance makes it more ordered and decreases its entropy. At absolute zero, the entropy of a perfect crystalline substance may be taken as zero. This statement is sometimes called the Third Law of Thermodynamics. On the basis of the third law, absolute entropies can be calculated from heat capacity data by extrapolating to absolute zero. Example : 2 Hg (l) + O2 (g) ® 2HgO (s) The third law entropies are S0 (Hg) = 18.5 Cal / 0K mole S0 (O2) = 49 Cal / 0K mole S0 (HgO) = 17.2 Cal / 0K mole D H0f (HgO) = - 21.68 K Cal / mole D S0 = - 51.6 Cal / 0K Now D H0 = 2 D H0f = - 43,400 Cal ( 2 moles ) \ D G0 = D H0 - TD S0 = - 43,400 - (298) (51.6) = - 28,000 Cal Since there is formation of two moles D G0f = -14.0 K Cal/mole ********** Index  