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| 7970304317 | differential rate laws | reveal the relationship between the concentration of reactants and the rate of the reaction | 0 | |
| 7970304318 | integrated rate laws | reveals the relationship between concentration of reactants and time | 1 | |
| 7970304319 | reaction rate | the change in concentration of a reactant or product per unit of time | 2 | |
| 7970304320 | differential rate law equation | rate=k[A]^m[B]^n | 3 | |
| 7970304321 | rate of appearance | change in [product] ---------------------------------- change in time (t2-t1) | 4 | |
| 7970304322 | rate of disappearance | change in [reactant] -------------------------------------- change in time(t2-t1) the rate at which one species disappears | 5 | |
| 7970304323 | Determination of reaction order | Experimentally from the data | 6 | |
| 7970304324 | zeroth order reactions | doubling the concentration has no effect on the rate at which this reaction occurs | 7 | |
| 7970304325 | first order reaction | doubling the concentration of that species doubles the rate of the reaction | 8 | |
| 7970304326 | second order reaction | doubling the concentration of that species quadruples the reaction rate; half-life doubles | 9 | |
| 7970304327 | how to find the overall rate of the reaction | determine the sum of the exponents in the rate law | 10 | |
| 7970304328 | factors affecting reaction rate | -surface area -concentration of reactants -temperature -nature of reactants (ie. solutions, gases) -catalysts (absence or presence of) | 11 | |
| 7970304330 | activated complex | the (temporary) structure created at the point of maximum energy along the reaction path; aka transition state | 12 | |
| 7970304331 | exothermic reaction | the potential energy of the REACTANTS is greater than that of the products | 13 | |
| 7970304332 | endothermic reaction | the potential energy of the PRODUCTS is greater than that of the reactants | 14 | |
| 7970304333 | activation energy | minimum energy required to start a reaction; energy at which successful collisions can occur | 15 | |
| 7970304336 | delta E | the energy lost or gained in a reaction (through work or heat or both) | 16 | |
| 7970304337 | kinetic control | thermodynamically favored processes that don't occur at measurable rates because of the high amount of activation energy needed for the reaction to take place | 17 | |
| 7970304338 | thermodynamically favoured | spontaneous | 18 | |
| 7970304339 | arrhenius equation | k=A^-Ea/RT | 19 | |
| 7970304340 | R | ideal gas constant | 20 | |
| 7970304341 | reaction mechanisms | the series of steps that sum to the overall reaction allows successful collisions to take place | 21 | |
| 7970304342 | unimolecular reactions | reactions that happen in one step | 22 | |
| 7970304343 | reaction intermediate | a substance that is produced and then consumed during the overall reaction | 23 | |
| 7970304344 | rate determining step | the slowest elementary step in a reaction | 24 | |
| 7970304345 | method of determining the rate law | Only through experimentation | 25 | |
| 7970304347 | termolecular reactions | these reactions are very rare and they require the simultaneous collision of 3 particles with sufficient energy and the correct orientation | 26 | |
| 7970304348 | catalyst | lowers the activation energy of a reaction; doesn't appear in the overall reaction | 27 | |
| 7970304349 | acid-base catalysis | the catalyst of the reaction is an acid or a base | 28 | |
| 7970304350 | surface catalysis | increases the number of collisions that have the correct orientation | 29 | |
| 7970304351 | enzyme | biological catalyst | 30 | |
| 7970304353 | units for k in a zero order reaction | M/s | 31 | |
| 7970304354 | units for k in a first order reaction | 1/s | 32 | |
| 7970304355 | units for k in a second order reaction | 1/Ms | 33 | |
| 7970304356 | units for k in a third order reaction | 1/M^2ᐧs | 34 | |
| 7970304357 | first order integrated rate law | ln[A]=-kt + ln[A]o | 35 | |
| 7970304358 | first order reaction graphs | plotting ln[A]t vs. time for first order reactions produce a straight line with a negative slope | 36 | |
| 7970304359 | half-life | the time it takes for the concentration of a reactant to decrease by half | 37 | |
| 7970304360 | half-life eqn (first order) | ln 2/k | 38 | |
| 7970304362 | 2nd order integrated rate law | 1/[A]=kt + 1/[A]o | 39 | |
| 7970304363 | graph for second order reactions | when plotting 1/[A]t vs. time, a straight line with a positive slope is produced | 40 | |
| 7970304364 | What is the only factor that can affect the activation energy of a reaction? | the addition of a catalyst | 41 | |
| 7970304365 | 4 ways to speed up a reaction | increase temperature increase surface area increase concentration add a catalyst | 42 | |
| 7970304367 | homogeneous catalyst | a substance that is consumed in one step of the reaction mechanism but is a product in a subsequent step | 43 | |
| 7970304368 | heterogeneous catalyst | a catalyst that exists in a difference phase from that of reactants and products | 44 | |
| 7970304369 | graph of zero order | plotting concentration vs. time producing a straight line and a negative slope | 45 | |
| 7971079243 | spontaneous reaction | thermodynamically favourable rxn (delta G is a negative value) | 46 | |
| 7973160921 | molecularity | number of molecules that participate as reactants in an elementary reaction | 47 | |
| 7973163331 | bimolecular reaction | reaction that involves the collision of two molecules | 48 | |
| 7973198567 | adsorption | binding of molecules to a surface (usually the first step in heterogeneous catalysis | 49 | |
| 7973221135 | multistep mechanism | consists of a sequence of elementary steps | 50 | |
| 7973233746 | decreases | reaction rate ___________ as Ea increases | 51 | |
| 7973748077 | method of initial rates | allows for determination of k, and order of reactants | 52 | |
| 7973752394 | order of a reactant | the exponent to which the [reactant] must be raised in the differential rate law | 53 |
