Chapter 4 Chemical Kinetics | CLASS 12TH | quick revision notes chemistry

Table of Contents

Class 12 Chemistry Revision Notes Chapter 4 Chemical Kinetics

Chemical kinetics: It is the branch of chemistry that deals with the study of reaction rates and their mechanisms.
Rate of reaction: It is the change in concentration of reactant (or product) in unit time.
The unit of rate of reaction is mol L-1s-1.
A + B → C + D
Rate of disappearance of $A = \frac{{ - d[A]}}{{dt}}$
where d[A] is small change in conc. of ‘A’ and dt is small interval of time
Rate of disappearance of $B = \frac{{ - d[B]}}{{dt}}$
Where d[B] is small change in conc. of ‘B’ and dt is small interval of time
Rate of appearance of $C = \frac{{ + d[C]}}{{dt}}$
Where d[C] is small change in conc. of ‘C’ and dt is small interval of time
Rate of appearance of $D = \frac{{ + d[D]}}{{dt}}$
Where d[D] is small change in conc. of ‘D’ and dt is small interval of time
Rate $Chemical Kinetics class 12 Notes Chemistry$
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.
Average rate: It is the rate of reaction measured over a long time interval.
Average rate $= \frac{{\Delta x}}{{\Delta t}}$
where is Δx change in concentration and Δt is large interval of time.
Instantaneous rate: It is the rate of reaction when the average rate is taken over a particular moment of time. Instantaneous rate $= \frac{{dx}}{{dt}}$ .
where dx is small change in conc. and dt is the smallest interval of time.
It is the expression which relates the rate of reaction with concentration of the reactants.
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.
The constant of proportionality ‘k’ is known as rate constant.
Molecularity of a reaction: The 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 and is never more than three. It cannot be zero.
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.
If rate law expression for a reaction is Rate = k [A]x [B]y
Then its order of reaction = x + y
Order cannot be determined with a given balanced chemical equation. It can be experimentally determined.
Integrated rate law for zero order reaction: R → P
$\frac{{dx}}{{dt}} = k{[R]^0}$
$k = \frac{{[{R_0}] - [R]}}{t}$
If we plot a graph between concentration of R vs time t, the graph is a straight line with slope equal to -k and intercept is equal to [Ro].
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 zero order reaction, the half-life time is ${t_{1/2}} = \frac{{[{R_0}]}}{{2k}}$
For first order reaction, the half-life time is ${t_{1/2}} = \frac{{0.693}}{k}$ , where ‘k’ is rate constant.
It is independent of initial concentration for first order reaction.
Rate law for first order reaction: R $\to$ P
$k = \frac{{2.303}}{t}\log \frac{{[{R_0}]}}{{[R]}}$
where ‘k’ is rate constant or specific reaction rate, [Ro] is initial molar conc., [R] is final molar conc. after time ‘t’.
$k = \frac{{2.303}}{t}\log \frac{a}{{a - x}}$
where ‘a’ is initial conc. reacted in time ‘t’ final conc., after time ‘t’ is (a – x).
If we plot a graph between ln[R] with time, we get a straight line whose slope = – k and intercept ln[Ro].
To calculate rate constant for first order gas phase reaction of the type
A(g) $\to$ B(g) + C(g)
$k = \frac{{2.303}}{t}\log \frac{{{p_1}}}{{(2{p_i} - {p_t})}}$
Where pi is initial pressure of A, pt is total pressure of gaseous mixture containing A , B, C
$p$ t = $p$ A + $p$ B + $p$ C
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.Example – Acidic hydrolysis of ester (ethyl acetate).
$C{H_3}COO{C_2}{H_5} + {H_2}O$ $\xrightarrow{{{H^ + }}}C{H_3}COOH + {C_2}{H_5}OH$
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.
Arrhenius equation of reaction rate: It gives the relation between rate of reaction and temperature.
$k = A{e^{ - {E_a}/RT}}$
$\ln k = \ln A - {E_a}/RT$
$\log k = \log A - \frac{{{E_a}}}{{2.303RT}}$
where k = rate constant, A = frequency factor, Ea = energy of activation R = gas constant, T = temperature in Kelvin,
$\log \frac{{{k_2}}}{{{k_1}}} = \frac{{{E_a}}}{{2.303R}}\left( {\frac{{{T_2} - {T_1}}}{{{T_1}{T_2}}}} \right)$
Probability factor or Steric factor
$Rate = P{Z_{AB}}.{e^{\frac{{ - {E_a}}}{{RT}}}}$
Where ZAB represents the collision frequency of reactants, A and B, ${e^{\frac{{ - {E_a}}}{{RT}}}}$ represents the fraction of molecules with energies equal to or greater than Ea and P is called the probability or steric factor.
Mechanism of reaction: It is the sequence of elementary processes leading to the overall stoichiometry of a chemical reaction.
Activated complex: It is an unstable intermediate formed between reacting molecules. Since, it is highly unstable and it readily changes into product.
Rate determining step: It is the slowest step in the reaction mechanism.
The number of collisions per second per unit volume of the reaction mixture is known as collision frequency (Z).