Match List I with List II

A-v, B-iv, C-ii, D-i

The correct answer is option 3. A-v, B-iv, C-ii, D-i.

Let us match the terms from List I with their corresponding descriptions from List II:

A. Arrhenius equation - v. \(k\text{ = }A.e^{\frac{-E_a}{RT}}\)

The Arrhenius equation relates the rate constant \((k)\) of a chemical reaction to the temperature \((T)\) and activation energy (Ea). It is expressed as \(k\text{ = }A.e^{\frac{-E_a}{RT}}\), where \(A\) is the pre-exponential factor, \(R\) is the gas constant, and \(T\) is the temperature in Kelvin.

B. The slowest step in the reaction mechanism - iv. Rate-determining step

The slowest step in a reaction mechanism determines the overall rate of the reaction. It is often referred to as the rate-determining step because the rate of the overall reaction cannot exceed the rate of this step.

C. The rate constant of a 2nd order reaction - ii. \(conc^{-1}\text{, }time^{-1}\)

For a second-order reaction, the rate constant \((k)\) is expressed as \(conc^{1−n}\, \ time^{-1}\), where \(conc\) represents concentration and \(n\) is the order of the reaction. For a second-order reaction, \(n\) is equal to \(2\), so the rate constant is \(conc^{-1}\, \ time^{-1}\).

D. The possibility of a reaction depends on - i. Free energy change

The possibility of a reaction occurring depends on the free energy change \((∆G)\) of the reaction. If \(∆G\) is negative, the reaction is spontaneous and likely to occur. If \(∆G\) is positive, the reaction is non-spontaneous and unlikely to occur.

Based on these matches, the correct option is: Option 1: A-v, B-i, C-ii, D-i