Chem 2 Exam 1, Ch 12

Front 1

reaction rate

Back 1

-reaction rate of a chemical reaction is defined as the change in concentration of a reactant or product per unit time:

Front 2

example of a reaction rate given a formula

Back 2

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.

Front 3

differential rate law

Back 3

-expresses how the rate depends on concentration

-aka rate law.

Front 4

integrated rate law

Back 4

-expresses how the concentrations depend on time.

Front 5

overall reaction order

Back 5

-sum of the orders for the various reactants

-ex from picture: n+m

Front 6

rate law, general

Back 6

Front 7

integrated first order rate law

Back 7

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

Front 8

half-life of a first order reaction

Back 8

ln(2) = 0.693

Front 9

integrated second order rate law

Back 9

-A plot of 1/[A] versus t will produce a straight line with a slope equal to k.

Front 10

half life of a second order reaction

Back 10

Front 11

integrated rate law for a zero order reaction

Back 11

a plot of [A] versus t gives a straight line of slope -k

Front 12

half life for a zero order reaction

Back 12

Front 13

summary of rate laws table

Back 13

Front 14

reaction mechanism

Back 14

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.

Front 15

intermediate

Back 15

-formed in a step in a reaction and consumed in a subsequent step

Front 16

elementary step

Back 16

a reaction whose rate law can be written from its molecularity

Front 17

molecularity

Back 17

the number of species that must collide to produce the reaction indicated by that step

Front 18

unimolecular step

Back 18

-reaction involving one molecule

-always first order overall

Front 19

bimolecular step

Back 19

-reaction involving the collision of two species of molecules

-always second order overall

Front 20

termolecular step

Back 20

-reaction involving the collision of three species of molecules

-rare, possibility of three molecules colliding simultaneously is very low

-always third order overall

Front 21

reaction mechanism and relation to elementary step, molecularity, and rate law table

Back 21

Front 22

rate determining step

Back 22

-slowest step

Front 23

how to form products

Back 23

Front 24

arrhenius equation

Back 24

A: frequency factor

R: 8.3145 J K mol

Front 25

value of R in arrhenius equation

Back 25

R = 8.3145 J K mol

Front 26

catalyst

Back 26

a substance that lowers the activation energy and speeds up a reaction

Front 27

adsorbtion

Back 27

collection of one substance on the surface of another substance

Front 28

absorbtion

Back 28

refers to the penetration of one substance into another