REACTION RATES & unit time, which results to an
increase in the reaction rate.
COLLISION THEORY: GROUP 1
B. TEMPERATURE
CHEMICAL KINETICS
- Chemical kinetics is the area of Most of the time, an increase in temperature
chemistry that tackles about speeds, is accompanied by an increase in the
or rates, at which chemical reactions reaction rate.
occurs.
C. MEDIUM OR STATE OF MATTER
RATE OF REACTION
- is the change in the molar The rate of a chemical reaction depends on
concentration of a reactant or a the medium in which the reaction occurs.
product per change in time.
D. PRESENCE OF CATALYSTS AND
rate = change in concentration COMPETITORS
change in time
Catalysts increase reaction rate by
Or m/s
promoting more effective collisions,
improving reactant orientation, weakening
internal bonds.
COLLISION THEORY
states that for a reaction to occur between E. PRESSURE
two particles:
Increasing the pressure of a reaction
a. The reacting particles must collide with improves the probability of the reactants to
each other. interact with each other, thus increasing the
rate of the reaction.
b. The reacting particles must collide with a
certain minimum energy called the However, this factor is important for
activation energy. Ea. Activation energy reactions involving gases only.
refers to the minimum energy required to
break the bonds for the reaction to take F. MIXING
place and new bonds of product to form.
Mixing the reactants increases their ability
c. The reacting particles collide in the to interact with each other, thus increasing
correct orientation. the rate of a chemical reaction.
FACTORS THAT INFLUENCE THE RATE
OF REACTION CONCLUSION
A. Concentration of Reactants: Chemical kinetics - The study of how fast
- A higher concentration of reactants chemical reactions happen and what affects
leads to more effective collisions per their speed.
, First-order ➜ rate changes directly
Reaction rate - How fast a reactant is used Second-order ➜ rate changes strongly
up or a product is formed in a chemical
reaction.
CATALYSIS: GROUP 3
Collision theory - The idea that particles Catalysis
must collide with enough energy and proper - is an action by catalyst which takes
orientation for a reaction to occur. part in a chemical reaction process
and can alter the rate of reactions,
Factors that influence reaction rate - and yet itself will return to its original
Conditions that can speed up or slow down form without being consumed or
a reaction, such as temperature, destroyed at the end of the
concentration, surface area, and the reactions. The process of pushing a
presence of a catalyst. reaction forward by lowering the
activation energy.
RATE LAW: GROUP 2
Rate law CATALYSIS ACTION
- is a way to measure and predict - REACTION KINETICS AND
reaction speed. MECHANISM
- is an equation that shows how the
reaction rate depends on the CATALYST
concentration of reactants. - A SUBSTANCE ADDED TO SPEED
UP THE RATE OF REACTION
It tells us: WITHOUT BEING CONSUMED.
How fast a reaction happens - SPEEDS UP REACTION, LOWERS
Which reactants affect the speed ACTIVE ENERGY, IS NOT
How changing concentration changes the CONSUMED, DOES NOT CHANGE
rate PRODUCT
Reaction Rate = speed at which reactants ACTIVATION ENERGY
turn into products. -THE ENERGY BARRIER: CATALYSIS
ALLOW A LARGER FRACTION OF
Measured by: EFFECTIVE COLLISION TO OCCUR AT A
The change in concentration over time GIVEN TEMPERATURE.
formula: INHIBITOR
Rate = ∆concentration / ∆time -A SUBSTANCE THAT COMBINES WITH
AN ENZYME AND PREVENTS IT FROM
Reaction Order TRIGGERING A REACTION
Reaction order = exponent in the rate
law. HETEROGENOUS, HOMOGENEOUS,
ENZYME CATALYSIS
Types:
Zero-order ➜ no effect of concentration
increase in the reaction rate.
COLLISION THEORY: GROUP 1
B. TEMPERATURE
CHEMICAL KINETICS
- Chemical kinetics is the area of Most of the time, an increase in temperature
chemistry that tackles about speeds, is accompanied by an increase in the
or rates, at which chemical reactions reaction rate.
occurs.
C. MEDIUM OR STATE OF MATTER
RATE OF REACTION
- is the change in the molar The rate of a chemical reaction depends on
concentration of a reactant or a the medium in which the reaction occurs.
product per change in time.
D. PRESENCE OF CATALYSTS AND
rate = change in concentration COMPETITORS
change in time
Catalysts increase reaction rate by
Or m/s
promoting more effective collisions,
improving reactant orientation, weakening
internal bonds.
COLLISION THEORY
states that for a reaction to occur between E. PRESSURE
two particles:
Increasing the pressure of a reaction
a. The reacting particles must collide with improves the probability of the reactants to
each other. interact with each other, thus increasing the
rate of the reaction.
b. The reacting particles must collide with a
certain minimum energy called the However, this factor is important for
activation energy. Ea. Activation energy reactions involving gases only.
refers to the minimum energy required to
break the bonds for the reaction to take F. MIXING
place and new bonds of product to form.
Mixing the reactants increases their ability
c. The reacting particles collide in the to interact with each other, thus increasing
correct orientation. the rate of a chemical reaction.
FACTORS THAT INFLUENCE THE RATE
OF REACTION CONCLUSION
A. Concentration of Reactants: Chemical kinetics - The study of how fast
- A higher concentration of reactants chemical reactions happen and what affects
leads to more effective collisions per their speed.
, First-order ➜ rate changes directly
Reaction rate - How fast a reactant is used Second-order ➜ rate changes strongly
up or a product is formed in a chemical
reaction.
CATALYSIS: GROUP 3
Collision theory - The idea that particles Catalysis
must collide with enough energy and proper - is an action by catalyst which takes
orientation for a reaction to occur. part in a chemical reaction process
and can alter the rate of reactions,
Factors that influence reaction rate - and yet itself will return to its original
Conditions that can speed up or slow down form without being consumed or
a reaction, such as temperature, destroyed at the end of the
concentration, surface area, and the reactions. The process of pushing a
presence of a catalyst. reaction forward by lowering the
activation energy.
RATE LAW: GROUP 2
Rate law CATALYSIS ACTION
- is a way to measure and predict - REACTION KINETICS AND
reaction speed. MECHANISM
- is an equation that shows how the
reaction rate depends on the CATALYST
concentration of reactants. - A SUBSTANCE ADDED TO SPEED
UP THE RATE OF REACTION
It tells us: WITHOUT BEING CONSUMED.
How fast a reaction happens - SPEEDS UP REACTION, LOWERS
Which reactants affect the speed ACTIVE ENERGY, IS NOT
How changing concentration changes the CONSUMED, DOES NOT CHANGE
rate PRODUCT
Reaction Rate = speed at which reactants ACTIVATION ENERGY
turn into products. -THE ENERGY BARRIER: CATALYSIS
ALLOW A LARGER FRACTION OF
Measured by: EFFECTIVE COLLISION TO OCCUR AT A
The change in concentration over time GIVEN TEMPERATURE.
formula: INHIBITOR
Rate = ∆concentration / ∆time -A SUBSTANCE THAT COMBINES WITH
AN ENZYME AND PREVENTS IT FROM
Reaction Order TRIGGERING A REACTION
Reaction order = exponent in the rate
law. HETEROGENOUS, HOMOGENEOUS,
ENZYME CATALYSIS
Types:
Zero-order ➜ no effect of concentration
