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Kinetics

Kinetics. Advanced Higher Chemistry Unit 2(f). The Rate Law. a A + b B → c C + d D. Rate  [A] m .[B] n. Rate = k [A] m .[B] n. Where… k = rate constant m and n = orders of reaction with respect to A and B. Orders of reaction.

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Kinetics

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  1. Kinetics Advanced Higher Chemistry Unit 2(f)

  2. The Rate Law aA + bB → cC + dD Rate  [A]m.[B]n Rate = k[A]m.[B]n Where… k = rate constant m and n = orders of reaction with respect to A and B

  3. Orders of reaction • Reactions usually occur in a series of steps. • The integers in the rate equation refer to the actual number of particles involved in the slowest step of the reaction. • This is the rate determining step.

  4. Ep Reaction pathway

  5. Example

  6. Calculating the Rate Constant • Can be calculated from a series of experiments in which the starting concentrations of reactants are varied…

  7. Example

  8. Reaction rates and reaction mechanisms

  9. Ep Reaction pathway

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