CHM 116 Study Guide - Collision Theory, Rate Equation, Equilibrium Constant
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Kinetics:many reactions require a high activation energy to react in a timely manner. 3 ways to measure rate: how fast the water disappears, how fast hydrogen is formed or how fast oxygen is formed. Rate = delta[o2]/delta time = delta[h2]/2delta time = - delta[h2o]/2delta time. Rate = k[a]x[b]y (x is reactant order of a y is reaction order of b) Over all reaction rate is respective orders summed. 2nd order will increase fate by whatever factor squared. Elementary reactions cannot be broken down into simpler steps. Orders do not have to be integers sometimes may be fraction. O3 o2 + o (fast) rate1 = k1[o3] O + o3 2o2 (slow) rate2 = k2[o][o3] The rate law of the whole reaction is the rate law of the slow step however in this case it is not an exceptable rate law because there is an intermediate. Catalysts: speeds up reactions without being used up biological catalysts are called enzymes.
