Column Column il R. Zero order reaction 1. t1 / 2 ∝(1)/([Ȧ]0) Q. First order reaction 2. t100 %=

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Column Column il R. Zero order reaction 1. t1 / 2...

Column Column il R. Zero order reaction 1. $t_{1 / 2} \propto \frac{1}{[\dot{A}]_{0}}$ Q. First order reaction 2. $t_{100 \%}=[A]_{0} / k$ R. Second order reactions 3. Involves at least two reactants S. Pseudo unimolecular reaction 4. $[A]=[A]_{0} e^{-k t}$ Code: (a) $\begin{array}{llll}P & Q & R & S \\ 2 & 1 & 4 & 2 \\ 2 & 4 & 1 & 3 \\ 2 & 1 & 3 & 4 \\ 3 & 2 & 1 & 4\end{array}$ (b) (c) (d)

Column Column il
R. Zero order reaction
1. $t_{1 / 2} \propto \frac{1}{[\dot{A}]_{0}}$
Q. First order reaction
2. $t_{100 \%}=[A]_{0} / k$
R. Second order reactions
3. Involves at least two reactants
S. Pseudo unimolecular reaction 4. $[A]=[A]_{0} e^{-k t}$
Code:
(a) $\begin{array}{llll}P & Q & R & S \\ 2 & 1 & 4 & 2 \\ 2 & 4 & 1 & 3 \\ 2 & 1 & 3 & 4 \\ 3 & 2 & 1 & 4\end{array}$
(b)
(c)
(d)

Key Concepts

Zero Order Kinetics

In zero order reactions, the rate of reaction is independent of the concentration of the reactant. The integrated rate law for a zero order reaction shows that the concentration decreases linearly with time. Moreover, the half-life of such a reaction is inversely proportional to the initial concentration, meaning that as the initial concentration increases, the time required for the concentration to reduce by half decreases.

First Order Kinetics

First order reactions have a rate that is directly proportional to the concentration of a single reactant. The integrated rate law of a first order reaction is characterized by an exponential decrease in concentration over time, leading to a half-life that is constant and independent of the starting concentration. This behavior is indicative of the exponential decay that defines first order processes.

Second Order Kinetics

In second order reactions, the rate is proportional either to the square of the concentration of one reactant or to the product of the concentrations of two reactants. These reactions typically involve interactions between two molecules or ions, and the integrated rate laws for second order reactions show a non-linear relationship between concentration and time. The treatment of second order kinetics often requires careful analysis to account for the stoichiometry of the interacting species.

Pseudo-unimolecular Reactions

Pseudo-unimolecular reactions arise when a reaction that is intrinsically more complex is simplified due to one reactant being present in a large excess. This allows the reaction to be treated as if it were first order with respect to the limited reactant. The resulting rate law and integrated form mimic those of a true first order reaction, making it easier to analyze kinetics under these conditions.

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