VI.1 Collision theory states that a reaction is most likely to occur if reactant particles collide with the proper energy and orientation. (3.4d)

VI.2 The rate of a chemical reaction depends on several factors: temperature, concentration, nature of reactants, surface area, and the presence of a catalyst. (3.4f)

VI.3 Some chemical and physical changes can reach equilibrium. (3.4h)

VI.4 At equilibrium the rate of the forward reaction equals the rate of the reverse reaction.The measurable quantities of reactants and products remain constant at equilibrium. (3.4i)

VI.5 LeChatelier’s principle can be used to predict the effect of stress (change in pressure, volume, concentration, and temperature) on a system at equilibrium. (3.4j)

VI.6 Energy released or absorbed by a chemical reaction can be represented by a potential energy diagram. (4.1c)

VI.7 Energy released or absorbed during a chemical reaction (heat of reaction) is equal to the difference between the potential energy of the products and the potential energy of the reactants. (4.1d)

VI.8 A catalyst provides an alternate reaction pathway, which has a lower activation energy than an uncatalyzed reaction. (3.4g)

VI.9 Entropy is a measure of the randomness or disorder of a system. A system with greater disorder has greater entropy. (3.1ll)

VI.10 Systems in nature tend to undergo changes toward lower energy and higher entropy. (3.1mm).