Match List I with List II:

Choose the correct answer from the options given below:

1.

A-II, B-IV, C-I, D-III

The correct answer is option 3. A-II, B-IV, C-I, D-III.

Let's break down each type of reaction and how they match with the given reactions.

1. First-Order Reaction

A first-order reaction is one where the rate of the reaction is directly proportional to the concentration of one reactant. In mathematical terms, if \( A \) is the reactant, the rate law can be expressed as:

\(\text{Rate} = k[A]\)

where \( k \) is the rate constant.

Example: Decomposition of \(N_2O_5\):

\(N_2O_5 \longrightarrow 2NO_2 + \frac{1}{2}O_2\)

This reaction is first-order with respect to \( N_2O_5 \). This means that the rate at which \( N_2O_5 \) decomposes depends on its concentration, and if you plot \(\ln[N_2O_5]\) versus time, you will get a straight line.

2. Zero-Order Reaction

A zero-order reaction is one where the rate of the reaction is independent of the concentration of the reactants. The rate law is given by:

\(\text{Rate} = k\)

where \( k \) is the rate constant.

Example:Decomposition of ammonia (\(2NH_3\)) on a platinum catalyst:

\(2NH_3\underset{\text{Pt catalyst}}{\overset{1130 K}{\longrightarrow}} N_2 (g) + 3H_2 (g)\)

In this reaction, the rate is controlled by the surface properties of the catalyst rather than the concentration of ammonia. Therefore, the reaction rate does not change with the concentration of \( NH_3 \), making it a zero-order reaction with respect to \( NH_3 \).

3. Pseudo-First-Order Reaction

A pseudo-first-order reaction occurs when a reaction that is fundamentally of a higher order behaves like a first-order reaction because one of the reactants is in such excess that its concentration effectively remains constant.

Example: Hydrolysis of sucrose in the presence of excess water:

\(C_{12}H_{22}O_{11} + H_2O \overset{H^+}{\longrightarrow} \underset{\text{Glucose}}{C_6H_{12}O_6} + \underset{\text{Fructose}}{C_6H_{12}O_6}\)

Here, water is in large excess compared to sucrose. Thus, the reaction rate depends primarily on the concentration of sucrose, making the reaction pseudo-first-order with respect to sucrose.

4. Second-Order Reaction

A second-order reaction has a rate that is proportional to the square of the concentration of one reactant or the product of the concentrations of two reactants. The rate law can be written as:

\(\text{Rate} = k[A]^2\)

or \(\text{Rate} = k[A][B]\)

Example: Saponification of ethyl acetate with sodium hydroxide:

\(CH_3COOC_2H_5 + NaOH \longrightarrow CH_3COONa + C_2H_5OH\)

This reaction is a classic example of a second-order reaction because it depends on the concentration of both ethyl acetate and sodium hydroxide.

Thus, the correct answer is option 3. A-II, B-IV, C-I, D-III