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Unit 7: Chemical Kinetics

Unit 7: Chemical Kinetics. Rates of Chemical R eactions Day 1. Reactant X. Unit 7: Kinetics. Reactant X. Product Y. What is Kinetics?. Kinetics is the study of the rate at which a reaction proceeds. Product Y. Reactant X. Product Y. Reactant X. Reaction Rates.

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Unit 7: Chemical Kinetics

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  1. Unit 7: Chemical Kinetics Rates of Chemical Reactions Day 1

  2. Reactant X Unit 7: Kinetics Reactant X Product Y What is Kinetics? Kinetics is the study of the rate at which a reaction proceeds Product Y Reactant X Product Y Reactant X Reaction Rates How fast can you drive? Product Y X Rate of reaction = Our First Example … Product Y X

  3. Unit 7: Kinetics Reactant Concentration vs. Time For the equation: X  Y Disappearance of reactant X Average “rate of disappearance” Instantaneous rates are normally used in chemistry. How fast is the reaction proceeding at t = 10 m?

  4. Unit 7: Kinetics Reactant Concentration vs. Time For the equation: X  Y Appearance of product Y Find the average “rate of appearance” of Y during the time interval of 5 – 10 minutes.

  5. Unit 7: Kinetics Reactant Concentration vs. Time This graph shows the concentration of a natural dye as a function of time. What is the average rate of change of the dye over the first 2 minutes? The last two minutes? X10-5

  6. Unit 7: Kinetics Relative Rates within a chemical reaction Stoichiometric coefficients can be used to compare the rates of disappearance of reactants to the rates of formation of products General Expression of reaction rate N2O5 2 NO2 + ½ O2

  7. Unit 7: Kinetics Relative Rates within a chemical reaction Stoichiometric coefficients can be used to compare the rates of disappearance of reactants to the rates of formation of products 4 PH3 P4 + 6H2 Relate the rates of disappearance and rates of formation for the previous reaction If the rate of formation of P4 is 0.25 mol/L∙min, what is the corresponding rate of disappearance of PH3?.

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