Save
GENCHEM 2ND SEM
( GENCHEM) KINETIC MOLECULAR THEORY
CHEMICAL KINETICS
Save
Share
Learn
Content
Leaderboard
Share
Learn
Created by
ai
Visit profile
Cards (19)
Learning
Objectives
Describe how various factors influence the rate of a reaction
Explain reactions
qualitatively
in terms of
molecular collisions
Identify the
order
of reactions
View source
Adding
heat
Increases
the rate of
reaction
View source
Removing heat
Decreases the rate of
reaction
View source
Adding a
catalyst
Increases
the rate of
reaction
View source
Diluting
a solution
Decreases
the rate of reaction
View source
Decreasing the surface area
Decreases
the rate of
reaction
View source
Increasing
the
concentration
Increases
the rate of
reaction
View source
Breaking a reactant down into smaller pieces
Increases
the rate of
reaction
View source
Colligative properties
Properties dependent on the number of
solute
particles dissolved in a given quantity of
solvent
View source
Examples of
colligative properties
Boiling point
Freezing point
View source
Factors affecting the rate of reaction
Nature
of reactants
Concentration
of reactants
Temperature
Surface area
Presence of a
catalyst
View source
Collision
theory
For a chemical reaction to occur, the
reacting
particles must
collide
with one another
Reacting particles often collided
without
reacting
For collision to be successful, reacting particles must collide with sufficient
energy
and proper
orientation
View source
Raising the reaction temperature by
10
⁰C can
double
or triple the reaction rate
View source
The reaction rate
decreases
with a
decrease
in temperature
View source
When solids and liquids react, increasing the
surface area
of the solid will
increase
the reaction rate
View source
Catalysts
can lower the activation energy and increase the
reaction rate
without being consumed in the reaction
View source
Reaction rate laws
Express the mathematical relationship between the rate of
reaction
and
concentration
of reactants
View source
Example experiment #1
Rate = K [A]^
1
[B]^
2
View source
Example experiment #
2
Rate =
K
[
F2
]^1 [ClO2]^1
View source