01:160:162 Lecture Notes - Lecture 8: Walther Nernst, Jmol, Enthalpy

• School: Rutgers University
• Department: Chemistry
• Course: 01:160:162
• Professor: Professor Klein- Juneau

Document Summary

Viii. boltzmann"s equation- a quantitative view of entropy (1844-1906: s = k*lnw, k- boltzmann constant. k = r/n = 1. 38 x 10^-23 j/k, w- the number of energetically equivalent ways to arrange the components of the system. Compressing an ideal gas at constant temperature: 4. ) Heating an ideal gas at constant pressure: 5. ) Xiii. interplay of ssystem and ssurroundings in determining the sign of suniverse: suniverse = ssystem + ssurroundings. Xiv. dependence on temperature- ssurroundings: heat flow (constant p) = change in enthalpy = h, ssurroundings = - h, an exothermic process increases the entropy of the surroundings, an endothermic process decreases the entropy of the surroundings. Xv. standard entropy values (s : s - designates standard state conditions, entropy is an extensive physical property of matter, represent the increase in entropy that occurs when a substance is heated from 0k to 298k at. Xviii. effect of h and s on spontaneity: g = h - t s.