How Chemical Reactions Occur
molecules must collide in order to react - a reaction proceeds faster if the concentrations for the reacting molecules are increased - reactions go faster at higher temperatures
A minimum energy called activation energy (Ea) is needed for a reaction to occur If a given collision possesses an energy greater than Ea, that collision can result in a reaction. If a collision has energy less than Ea, the molecules will bounce apart unchanged At higher temperatures the average collision is more energetic
A catalyst can speed up a reaction without being consumed in the overall reaction Enzymes are catalysts in our bodies that help speed up complicated reactions that would be too slow to sustain life at normal body temp. A catalyst works because it provides a new pathway for the reaction- a pathway that has a lower activation energy than the original pathway (more collisions will have enough energy to allow a reaction)
Homogeneous reaction- involves reactants and products in one phase of matter Heterogeneous reaction- involves reactants and products in two phases of matter -The speed of a reaction depends on the surface area available -surface area effects the explosive combustion of grain dust
Chemists define equilibrium as the exact balancing of two processes, one of which is the opposite of the other. ( page 601) The equilibrium state occurs when the rate of evaporation exactly equals the rate of condensation There are many chemical reactions that “stop” far short of completion when they are allowed to take place in a closed container.
Chemical equilibrium is a dynamic state where the concentrations of all reactants and products remain constant, as long as the conditions are not changed. Chemical reactions that are reversible, they can occur in either direction, are indicated by double arrows. Pg 602
Equilibrium is not static but is a highly dynamic situation- it may appear everything has stopped but on the molecular level there is frantic activity