CHEMICAL KINETICS CHEMICAL KINETICS CHEMICAL KINETICS The applications of chemistry mainly focus on chemical reactions. ►Need to know several of its characteristics:  Stoichiometry  Energetics  Rate CHEMICAL KINETICS The area of chemistry that concerns reaction rates is called chemical kinetics < TARGET="display"> < TARGET="display"> < TARGET="display"> < TARGET="display"> < TARGET="display"> < TARGET="display"> [...]... a Reaction CH3Br (aq) + OH-(aq) → CH3OH(aq) + Br -( aq) Rate = k(CH3Br)(OH-) (CH3)3CBr(aq) +OH-(aq) → (CH3)3COH(aq) + Br-(aq) Rate = k((CH3)3CBr) ► The rate law for a reaction cannot be predicted from the stoichiometry of the reaction; it must be determined experimentally The Rate Law Versus the Stoichiometry of a Reaction 2 HI(g) → H2(g) + I2(g) Rate = k(HI)2 2 N2O5(g) → 4 NO2(g) + O2(g) Rate = k(N2O5) . ( Br ( aq aq ) + OH ) + OH - - ( ( aq aq ) ) → → CH CH 3 3 OH( OH( aq aq ) + Br ) + Br - - ( ( aq aq ) ) Rate = Rate = k k (CH (CH 3 3 Br)(OH Br)(OH - - ) ) (CH (CH 3 3 ) ) 3 3 CBr( CBr( aq aq ). k k (CH (CH 3 3 Br)(OH Br)(OH - - ) ) (CH (CH 3 3 ) ) 3 3 CBr( CBr( aq aq ) +OH ) +OH - - ( ( aq aq ) ) → → (CH (CH 3 3 ) ) 3 3 COH( COH( aq) aq) + Br + Br - - ( ( aq aq ) ) Rate = k((CH Rate = k((CH 3 3 ) ) 3 3 CBr) CBr) . I 2 2 ( ( g g ) ) Rate = Rate = k k (HI) (HI) 2 2 2 N 2 N 2 2 O O 5 5 ( ( g g ) ) → → 4 NO 4 NO 2 2 ( ( g g ) + O ) + O 2 2 ( ( g g ) ) Rate = Rate = k k (N (N 2 2 O O 5 5 ) )