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28 Cards in this Set
- Front
- Back
reaction rate |
-reaction rate of a chemical reaction is defined as the change in concentration of a reactant or product per unit time: |
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example of a reaction rate given a formula |
In the balanced equation, the product O2 has a coefficient of 1, which means it is produced half as fast as NO, since NO has a coefficient of 2. That is, the rate of NO production is twice the rate of O2 production. |
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differential rate law |
-expresses how the rate depends on concentration -aka rate law. |
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integrated rate law |
-expresses how the concentrations depend on time. |
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overall reaction order |
-sum of the orders for the various reactants -ex from picture: n+m |
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rate law, general |
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integrated first order rate law |
y=mx+b -reaction is first order in A if a plot of ln[A] versus t is a straight line -k is the slope of your line |
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half-life of a first order reaction |
ln(2) = 0.693 |
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integrated second order rate law |
-A plot of 1/[A] versus t will produce a straight line with a slope equal to k. |
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half life of a second order reaction |
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integrated rate law for a zero order reaction |
a plot of [A] versus t gives a straight line of slope -k |
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half life for a zero order reaction |
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summary of rate laws table |
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reaction mechanism |
series of steps in a chemical reaction, satisfies two requirements: 1. The sum of the elementary steps must give the overall balanced equation for the reaction. 2. The mechanism must agree with the experimentally determined rate law. |
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intermediate |
-formed in a step in a reaction and consumed in a subsequent step |
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elementary step |
a reaction whose rate law can be written from its molecularity |
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molecularity |
the number of species that must collide to produce the reaction indicated by that step |
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unimolecular step |
-reaction involving one molecule -always first order overall |
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bimolecular step |
-reaction involving the collision of two species of molecules -always second order overall |
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termolecular step |
-reaction involving the collision of three species of molecules -rare, possibility of three molecules colliding simultaneously is very low -always third order overall |
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reaction mechanism and relation to elementary step, molecularity, and rate law table |
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rate determining step |
-slowest step |
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how to form products |
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arrhenius equation |
A: frequency factor R: 8.3145 J K mol |
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value of R in arrhenius equation |
R = 8.3145 J K mol |
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catalyst |
a substance that lowers the activation energy and speeds up a reaction |
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adsorbtion |
collection of one substance on the surface of another substance |
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absorbtion |
refers to the penetration of one substance into another |