Kinetics

Step 1: Difference Between Molecularity and Order: \begin{center} \begin{tabular}{|c|c|} \hline Molecularity & Order of Reaction
\hline It is the number of molecules colliding in an elementary step. & It is determined experimentally from rate law.
\hline Always a whole number. & Can be fractional or whole.
\hline \end{tabular} \end{center} Step 2: First-Order Reaction Derivation: For three-fourth completion: Thus, the time taken for 75% completion is twice the half-life.

Step 1: Effect of Temperature: - Higher temperature increases reaction rate by providing activation energy.
- Follows Arrhenius equation: Step 2: First-Order Reaction Calculation: Given: 20\% completion in 10 minutes. For 80\% completion: Thus, the time required for 80\% completion is 72.2 minutes.

- First-order Reaction: The rate of reaction depends on the concentration of a single reactant. The rate law is: - Half-life ( ): For a first-order reaction: Calculation: