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| 12838901374 | mechanism | series of elementary steps that make up an overall reaction | 0 | |
| 12838901375 | intermediate | does not appear in the overall reaction (is created and consumed in overall reaction). | 1 | |
| 12838901376 | rate-determining step | slowest step in the mechanism. determines overall reaction rate | 2 | |
| 12838901377 | collision theory | the rate of a reaction is proportional to the number of collisions per second between reacting molecules | 3 | |
| 12838901378 | an effective collision occurs when... | molecules collide at the correct orientation and have sufficient energy | 4 | |
| 12838901379 | activation energy | the minimum energy of collision necessary for a reaction to take place. (Ea) the energy required to reach the transition state | 5 | |
| 12838901405 | Arrhenius equation, which embodies collision theory |  | 6 | |
| 12838901380 | frequency factor | measure of how often molecules in the reaction collide (A) | 7 | |
| 12838901381 | As temperature increases, the rate constant... | increases | 8 | |
| 12838901382 | the frequency factor can be increased by... | the number of molecules/concentration | 9 | |
| 12838901383 | transition state | old bonds are weakened and new bonds are beginning to form. highest energy state. |  | 10 |
| 12838901384 | transition states vs intermediates | transition states are theoretical constructs that exist at the point of max energy. | 11 | |
| 12838901385 | 4 factors that affect reaction rate | concentrations, temperature, medium, catalyst | 12 | |
| 12838901386 | as reactant concentrations increase, reaction rate.... | increases (more mlcs, more collisions, higher frequency factor) UNLESS its a zero-order reaction | 13 | |
| 12838901387 | as temperature increases, reaction rate.... | increases (more kinetic energy, more mlcs with enough energy to surpass Ea) BUT too much heat may cause a catalyst to denature. | 14 | |
| 12838901388 | how does medium affect reaction rate? | some mlcs are more likely to react in an aqueous or non-aqueous solvent. physical state can also have an effect. Typically, polar solvents are preferred because mlcr dipole tends to polarize and weaken bonds of reactants, making reaction go faster | 15 | |
| 12838901389 | catalyst | substance that increases reaction rate without being consumed in the reaction, interact with reactants by absorption or creation of intermediates, stabilizing them and reducing activation energy. | 16 | |
| 12838901390 | homogeneous catalysis | catalyst is in the same phase (solid, liquid, gas) | 17 | |
| 12838901391 | heterogeneous catalysis | catalyst is in a different phase (solid, liquid, gas) | 18 | |
| 12838901392 | limitations of catalysts | cant effect the free energies of reactants or products cant effect the equilibrium position or Keq | 19 | |
| 12838901393 | rate law expression | k= rate constant m,n= orders of reactants measured in M/s determined experimentally |  | 20 |
| 12838901394 | zero-order reaction | rate of formation of the product is independent if the changes in concentration of the reactants. only way to change the rate of a zero-order reaction is with a catalyst |  | 21 |
| 12838901395 | first order reaction | rate is directly proportional to only one reactant. |  | 22 |
| 12838901396 | second order reaction | rate is proportional to either two reactants or the square concentration of one. |  | 23 |
| 12838901397 | mixed-order reaction | non integer orders | 24 | |
| 12838901398 | plotting a first order reaction | Ln[A]t=-kt+Ln[A]o y=mx+b y axis: Ln[A] x axis: t slope: -k linear graph | 25 | |
| 12838901399 | half-life | time to get to half the initial concentration | 26 | |
| 12838901406 | half-life of a first order reaction |  | 27 | |
| 12838901400 | plotting a second order reaction | 1/[A]t=kt+1/[A]o y axis: 1/[A] x axis: t slope: k | 28 | |
| 12838901407 | half life of a second order reaction |  | 29 | |
| 12838901401 | molar absorptivity in spectroscopy | a measure of how well a chemical species absorbs a given wavelength of light | 30 | |
| 12838901402 | 0% transmittance in spectroscopy | If all the light is absorbed in a solution | 31 | |
| 12838901403 | The average rate of disappearance of ozone in the reaction 2O3 --> 3O2 is found to be 8.76 × 10¯3 atm over a certain interval of time. What is the rate of appearance of O2 during this interval? | 13.1 × 10¯3 atm/s | 32 | |
| 12838901404 | What's the rate law for: X → Y + Z | Rate = k[X] | 33 |
