Collision Theory Of Chemical Reactions

Step 1: General rate law: $ \mathrm{CHCl_3}=1 \mathrm{Cl_2}=\frac12 $

Step 1: Rate law: $ =6\times10^{-4} [A]=0.3 k $

Concept: For a first-order reaction, the rate of reaction depends linearly on the concentration of the reactant. The integrated rate law for a first-order reaction is: where
• = initial concentration
• = concentration at time
• = rate constant
• = time The half-life is the time required for the concentration of the reactant to become half of its initial value.

Step 1: Definition of half-life. For half-life, Substitute this in the first-order rate equation:

Step 2: Evaluating the logarithmic value. Therefore,