CHM 101 Lecture Notes - Lecture 6: Exothermic Reaction, Endothermic Process, Heat Transfer
Document Summary
Heat: transfer of energy due to temperature difference. Surroundings: part of the universe not being studied. Heat goes from system to surrounding q is exothermic: - Heat goes from surroundings into the system q is endothermic: + State of a system: describes macroscopic properties of a system. State functions: properties that are determined by the state of the system. Path functions: path from initial state affects the value. Change in internal energy of a system= u =ufinal uinitial. Consider: s(s) + o2 (g) so2 (g) = energy content of 1 mol so2(g) energy content of (1 mol s(s) + 1 mol o2(g) 1st law of thermodynamics: energy can be converted from 1 form to another by cannont be created or destroyed. Pv= force/area x volume = f/d2 x d3 = fd = w. Negative work (w < o): system does work on surroundings. Positive work (w > 0): work done on system by surroundings.
