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Chem 113- Unit 1
| Question | Answer |
|---|---|
| four controllable factors for reaction rate | concentration, physical state, temperature, catalyst |
| initial rate | rate (t=0) = Δ[A]/Δt |
| zero order | rate=k |
| first order | rate=k[A] |
| second order | rate=[A]^2 |
| overall reaction order | the sum of all reaction orders |
| first order integrated rate law | ln[A]t=-kt+ln[A]0 |
| second order integrated rate law | 1/[A]t=kt+1/[A]0 |
| zero order integrated rate law | [A]t= -kt +[A]0 |
| Arrhenius equation | K=Ae^(-Ea/RT) |
| Arrhenius equation (for T1/T2) | ln (k2/k1)= (-Ea/R)(1/T2-1/T1) |
| ΔH (rxn)= | Ea(fwd)-Ea(rev) |
| if temp is held constant... | higher Ea= lower f |
| if Ea is held constant... | higher temp= higher f |
| transition state | symbolized by the activation state-> could go back to reactants or to products |
| reaction intermediates | created and used up in elementary steps |
| unimolecular (elementary step) | first order, rate=k[A] |
| bimolecular (elementary step) | 2nd order, rake=k[A]^2 |
| termolecular (elementary step) | ***not likely to occur 3rd order, rate=k[A]^3 |
| rate determining step | (RDS) highest energy step; slowest step |
Created by:
melaniebeale
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