1. ENTROPY AND CHEMICAL REACTIONS

2. SPONTANEITY  Basically the law of conservation of energy  energy can be neither created nor destroyed  i.e., the energy of the universe is constant  the total energy is constant  energy can be interchanged  e.g. potential energy (stored in chemical bonds) can be converted to thermal energy in a chemical reaction  CH 4 + O 2 --> CO 2 + H 2 O + energy  Doesn’t tell us why a reaction proceeds in a particular direction

3. ENTROPY Randomness or disorder of a system. Increases as temperature increases Increases as you increase agitation Increases as you add energy to the system

4. ENTROPY  Symbol: S  A measure of randomness or disorder  The natural progression is from order to disorder  It is natural for disorder to increase  Entropy is a thermodynamic function  Describes the number of arrangements that are available to a system in a given state

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6. ENTROPY  The greater the number of possible arrangements, the greater the entropy of a system, i.e., there is a large positional probability.  The positional probability or the entropy increases as a solid changes from a liquid or as a liquid changes to a gas