These are Online Short Notes on Chapter 4 (Chemical Kinetics) For Practice of CBSE Board, CBSE NEET, CSIR NET etc.1. Chemical kinetics: The branch of chemistry that deals with the study of
reaction rates and their mechanisms is called chemical kinetics.
2. Rate of reaction: It is defined as the change in concentration of reactant (or product) in unit time. Unit of rate of reaction is mol L-1s-1.
3. Average rate: The rate of reaction measured over a long time interval is called average rate of reaction. It is equal to Δx/Δt.
4. Instantaneous rate: It is the rate of reaction when the average rate is taken over a particular moment of time. It is equal to dx/dt.
5. Rate law or rate equation: It is the expression which relates the rate of reaction with concentration of the reactants. The constant of proportionality ‘k’ is known as rate constant.
6. Rate constant: When the concentration of reactants is unity, then the rate of reaction is known as rate constant. It is also called specific reaction rate.
7. Molecularity of a reaction: Total number of atoms, ions or molecules of the reactants involved in the reaction is termed as its molecularity. It is always in whole number. It is never more than three. It cannot be zero.
8. Order of a reaction: The sum of the exponents (power) of the concentration of reactants in the rate law is termed as order of the reaction. It can be in fraction. It can be zero also.
9. Half- life of a reaction: The time taken for a reaction, when half of the starting material has reacted is called half- life of a reaction. For first order reaction
t1/2 = 0.693/k ,where k is rate constant.
It is independent of initial concentration for first order reaction.
10. Pseudo first order reaction: The reaction which is bimolecular but order is one is called pseudo first order reaction. This happens when one of the reactants is in large excess. E.g., acidic hydrolysis of ester (ethyl acetate).
CH3COOC2H5 + H2O ==H+==> CH3COOH + C2H5OH
11. Activation energy (Ea): It is extra energy which must be possessed by reactant molecules so that collision between reactant molecules is effective and leads to the formation of product molecules.
12. Arrhenius equation of reaction rate: It gives the relation between rate of reaction and temperature.
k =Ae -Ea /RT
where k = rate constant, A = frequency factor,
Ea = energy of activation
R = gas constant, T = temperature in Kelvin,
ln k = ln A - Ea/RT
log k = [ log A - ( Ea / 2.303 RT ) ]
13. Mechanism of reaction: The sequence of elementary processes leading to the overall stoichiometry of a chemical reaction is known as mechanism of a reaction.
14. Activated complex: It is defined as unstable intermediate formed between reacting molecules. It is highly unstable and readily changes into product.
15. Rate determining step: The slowest step in the reaction mechanism is called rate determining step.
16. Collision Frequency (Z):The number of collisions per second per unit volume of the reaction mixture is known as Collision Frequency (Z).
No comments:
Write comments