Chapter 13: Kinetics: Mechanisms and Rates of Chemical Reactions
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36 terms
Terms | Definitions |
|---|---|
 Way to determine rate of overall chemical reaction | Determined by rates of elementary reactions |
| Rate determining step | Elementary rxn that proceeds slower than any of other steps in mechanism. Governs rate of overall chem rxn. |
| kinetics | study of rates of chem rxns |
| kinetic units | M/s-1 |
| The reason stoichiometry isn't used for rate law for a reaction. | because orders must be determined experimentally |
| Cases where stoichiometry is acceptable to determine rate law. | Single elementary steps and rate limiting steps. |
| Three concepts of reaction mechanisms and rate laws. | . Mechanism is one or more elementary reaction that describes how chem reaction occurs sum of individual steps of mechanism gives balanced stoichiometric chem equation rate law predicted by mechanism is same as experimental rate law. |
| Units for zero order | Ms-1 |
| units for first order | s-1 |
| units for second order | M-1s-1 |
| specific heat of water? | 4.184 C |
| (5/9)(f-32) | F to C |
| concentration reactant at the beginning, concentration remaining at time t, and rate constant. | In the Order reaction equations what does [A]o, [A], and kt stand for? |
| first order | the linear order |
| ln([A]o/[A])=kt | first order reactant eqn |
| Half life | amount of time required for half the amount of reactant to be consumed |
| the original concentration, [A]o | In first order reactions, what is half life independent of? |
| t(1/2)=ln2/k | WHAT'S HALF LIFE FORMULA? |
| reciprocal of concentration varies linearly with time | second order reaction graph |
| concentration varies linearly with time | zero order |
| By examining how concentration changes | how can rate laws be determined? |
| unimolecular fragmentation | energy of products is always higher than that of reactants |
| unimolecular rearrangement | the energy always rises initially, but as bond forms, energy decreases. |
| 0.0821, 8.314 | the two "R" constants |
| reaction mechanism | Sequence of molecular events |
| molecular event during chem rxn with 1-3 reactants | Elementary reactions |
| Most common elementary reaction. Collision of two reactants | bimolecular reaction |
| unimolecular reaction | Elementary reaction where a single molecule breaks into two pieces and rearranges into a new isomer |
| termolecular reaction | Elementary reaction where three chem species collide simultaneously. Very rare. |
| Chemical species produced in early step of a mechanism and consumed in a later step. Never appears in overall reaction. | Intermediates |
| molecular events/time | Define rate of reactions |
| Rate determining step | elementary rxn that procedes more slowly than any other step in mechanism. Governs overall chem rxn. |
| kinetics | study of rates of chem rxns. |
| units of kinteics | Ms-1 |
| unimolecular rxns slow down | When less reactant molecules remain. |
| rate=k[A]x[B]y | rate law skeleton |
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