Rates of Reaction
Rate of reaction : the speed at which reactants turn into products
Slow reaction Moderate reaction Fast reaction
the rusting of iron metal magnesium reacting with explosions/fireworks
↳ (years/decades) an acid to produce a gentle ↳ La fraction of a second
stream of bubbles
↳ (minutes
grams's grams's
Rate of reaction Quantity of products formed Rate of reaction Quantity of reactants used
Time taken Time taken
S S
f
m-
faster Steeper line faster
vol. of product produced
products
=
,
more
and more reactants reaction
m-
the line gradually
faster reaction with
becomes less steep as
the same amount of
the reactants are used up
reactants
m-
original reaction
time (s)
Covision Theory
The rate of a chemical reaction depends Om :
1) The collision frequency (double frequency of collisions , double the rate)
2) Energy transferred during a collision (particles need enough energy for a successful
collision
Activation energy : the minimum amount of energy particles need to react
↳
greater activation energy more energy needed to start the reaction
↳ this must be supplied (e
.g. heating
increasing the number of collisions ,
increases the rate of reaction
Factors that affect the rate of chemical reaction
1) Temperature 2 Concentration (/pressure
.
. Surface
3 Area
COLD HOT
increase
D-
&
& &
1 . increased temperature = more more concentrated =
more breaking a solid reactant into
Kinetic energy (for particles reactant particles in the smaller pieces increases the surface
2 increased same volume area to volume ratio
.
.
temperatures = - >
making
increased energy of collisions collisions more likely +
↳
surrounding particles have more
area to work on and the
: more successful collisions increasing the rate of
frequency of collisions increase
+
reaction
at higher temperatures increase in rate of reaction
.
Rate of reaction : the speed at which reactants turn into products
Slow reaction Moderate reaction Fast reaction
the rusting of iron metal magnesium reacting with explosions/fireworks
↳ (years/decades) an acid to produce a gentle ↳ La fraction of a second
stream of bubbles
↳ (minutes
grams's grams's
Rate of reaction Quantity of products formed Rate of reaction Quantity of reactants used
Time taken Time taken
S S
f
m-
faster Steeper line faster
vol. of product produced
products
=
,
more
and more reactants reaction
m-
the line gradually
faster reaction with
becomes less steep as
the same amount of
the reactants are used up
reactants
m-
original reaction
time (s)
Covision Theory
The rate of a chemical reaction depends Om :
1) The collision frequency (double frequency of collisions , double the rate)
2) Energy transferred during a collision (particles need enough energy for a successful
collision
Activation energy : the minimum amount of energy particles need to react
↳
greater activation energy more energy needed to start the reaction
↳ this must be supplied (e
.g. heating
increasing the number of collisions ,
increases the rate of reaction
Factors that affect the rate of chemical reaction
1) Temperature 2 Concentration (/pressure
.
. Surface
3 Area
COLD HOT
increase
D-
&
& &
1 . increased temperature = more more concentrated =
more breaking a solid reactant into
Kinetic energy (for particles reactant particles in the smaller pieces increases the surface
2 increased same volume area to volume ratio
.
.
temperatures = - >
making
increased energy of collisions collisions more likely +
↳
surrounding particles have more
area to work on and the
: more successful collisions increasing the rate of
frequency of collisions increase
+
reaction
at higher temperatures increase in rate of reaction
.
