reaction kinetics
DESCRIPTION
Reaction Kinetics. The rate at which a reaction occurs. Kinetic Energy. Related to molecular speed KE= ½ mv 2 Higher velocity (faster)= higher energy. Reaction Rate. The rate of reaction tells the speed at which the reaction takes place. Collision Theory. - PowerPoint PPT PresentationTRANSCRIPT
Reaction KineticsThe rate at which a reaction occurs
Related to molecular speed KE= ½ mv2
◦ Higher velocity (faster)= higher energy
Kinetic Energy
The rate of reaction tells the speed at which the reaction takes place
Reaction Rate
Collision Theory states that atoms, ions, and molecules must collide in order to react
Collision Theory
Not every collision between atoms and molecules results in a reaction!
1. Orientation is critical! 2. They must collide with sufficient energy
(the activation energy)
Collision Theory
CO (g) + NO2 (g) CO2 (g) + NO (g)
Any change that increases the number of collisions should increase the reaction rate
Collision Theory
Factors in reaction rates…
What are their tendencies towards bond formation?◦ Cs + H2O -----> CsOH + H2
Instantaneous◦ Cs very reactive(low IE, EN)◦ Fe + H2O -----> Fe2O3+ H2
very slow
1. Nature of the reactants
Reactions usually occur in liquid, gas, or aqueous phase
Related to surface area◦ Higher surface area means faster reaction in
heterogeneous reactions Reactions only occur at phase interface
2. The ability of the reactants to meet (collide)
Often listed as molarity (mol/L) Written as square brackets [ ]
◦ The moalrity (concentration) of HBr= [HBr] More reactants = more collisions More collisions = increases reaction rate
3. Concentration of the reactants
Temperature is a measure of average kinetic energy
Higher T means higher KE Faster moving molecules means more
collisions More collisions means a faster reaction rate
4. Temperature
4. Temperature
Increases the reaction rate without being consumed in the process
Lower the energy needed to react (Ea)
5. Catalyst
Lower activation energy means more collisions between particles have sufficient energy to react.
5. Catalyst
A heterogeneous catalyst exists in a physical state different than that of the reaction it catalyzes.
A homogeneous catalyst exists in the same physical state as the reaction it catalyzes.
A reforming catalyst is consumed in the reaction, but then re-made
An enzyme is a biologically active catalyst An inhibitor slows down a reaction by
increasing the activation energy
5. Catalyst
1. Nature of the reactants2. The ability of the reactants to collide3. The concentration of the reactants4. The temperature5. Catalysts
To review….
Now with numbers…
A rate is something per unit of time◦ interest rate = $ earned / time ◦ speed = distance traveled/ time ◦ pay = dollars / hour
Measuring rates
as the reaction proceeds, the reactants are “used up”
[reactants] goes down [products] goes up Reaction rate is measured as :
◦ Δconcentration /Δtime •(mol/L)/s, M/s, or mol L-1s-1
Measuring reaction rates
Graphing ΔM
The coefficients of a chemical equation give us some insight as to the relative rates of consumption of reactants and production of products, but not “absolute” amounts.
Coefficients and Rates
It takes 2 A’s for every single B that reacts, so A is “disappearing” twice as fast as B is
2A + B 3C + 2D
There are 2 D’s produced for every B and every 2 A’s that are “consumed”, so D is appearing at the same rate A is disappearing and twice as fast as B is disappearing
2A + B 3C + 2D
C is being produced 3 times faster than B is being used up, and 3/2 times faster that A is being used up
2A + B 3C + 2D
A Rate Lawis an equation that describes how a change in concentration affects the reaction rate.◦ for the reaction A + B products◦ The rate law would be: ◦ rate = k[A]m[B]n
Rate Law
rate = k[A]m[B]nk= the rate constant depends on the
temperature, different for each reaction
m= the “order of reaction” with respect to A
n= the “order of reaction” with respect to B
Rate Law
rate = k[A]m[B]n m and n have to be experimentally
determined; they are not the same as the reaction coefficients except by coincidence.
Rate Law