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Chemistry AP: Kinetics Practice

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Section 1

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reaction mechanisms

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Chemistry Science

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Date created

Mar 1, 2020

Cards (30)

Section 1

(30 cards)

reaction mechanisms

Front

a series of steps that make up the overall reaction

Back

1st order K units

Front

k = 1/time

Back

Increasing the concentration by 2 has no effect on the rate

Front

zero order

Back

concentration

Front

more particles; greater number of collisions

Back

Exothermic reactions

Front

Potential energy of reactants is greater that potential energy of products

Back

first order graph straight

Front

ln[ ]

Back

Increasing the concentration by 2 quadruples the rate

Front

second order

Back

catalyst

Front

1) a substance that speeds up a reaction by lowering the activation energy barrier 2) not a product or reactant; is not used or changed

Back

rate law

Front

expresses how the reaction rate of a particular reaction is dependent upon the concentrations of its reactants

Back

M

Front

moles per liter

Back

rate units

Front

molarity/time (M/s)

Back

m and n

Front

order of reactants

Back

[ ]

Front

concentration in molarity

Back

[A] and [B]

Front

concentration of reactants in moles per liter (M)

Back

reaction rate

Front

the change in concentration of a reactant or product per unit time

Back

second order graph straight

Front

1/ [ ]

Back

rate law general form

Front

rate = k [A]^m [B]^n

Back

k

Front

specific rate constant

Back

temperature

Front

1) reactions go faster at higher temperatures 2) particles have more kinetic energy 3) more colliding particles have enough energy to overcome activation energy barrier

Back

sum of m and n

Front

order of the reaction

Back

0 order K units

Front

k= M/s

Back

Endothermic

Front

Potential energy of reactants is less than that potential energy of products

Back

factors that affect reaction rate

Front

1) temperature 2) concentration 3) particle size 4) catalyst

Back

Increasing the concentration by 2 doubles the rate

Front

first order

Back

2nd order K units

Front

k = 1/ Ms

Back

intermediate

Front

the product of 1 step of a reaction that immediately becomes a reactant in the next step

Back

rate limiting/rate determining step

Front

the slowest step in a reaction that determines how fast the reaction can go and has the highest activation energy

Back

particle size

Front

more surface area; more collisions

Back

activation energy

Front

2 or more particles must collide with sufficient energy and proper molecular orientation in order to react

Back

3rd order K units

Front

k = 1/M^2 s

Back