CHEM 6B Lecture Notes - Lecture 11: Heat Capacity, Calorimetry, Exothermic Process
9 Feb 2017
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Document Summary
State- measurable properties (vol, pressure, temp) that define a system. Process- path the system takes (initial-final state) Energy- capacity to do work or transfer heat. Potential energy- energy a body possesses on account of its position in a field of force. (ep=m*g*h) Internal energy- denoted as e or u, total capacity of a system to do work. Change in internal energy- e = efinal - einitial. When transfer of energy is only as work= e = w. When work is done by system (w<0), when done on system (w>0) Heat-denoted by (q), energy transferred as result of temp change. Energy flows from high temp to low temp. When only transfer of energy is heat (cid:857) (cid:902) (cid:878) (cid:930)(cid:858) If energy leaves system (q<0), if it enters (q>0) Heat is in almost all chemical reactions. Endothermic- when reaction absorbs heat from surroundings. Exothermic- when reaction is accompanied by release of heat to surroundings. Closed system- exchange of energy but not matter.
