Chapter 14, Problem 91SCQ

Interpretation Introduction

Interpretation:

For the given set of statements it should be identified that whether they are true or false and the false the statements are should be corrected.

Concept introduction:

Collision theory: The rate for the reaction is predicted by using collisions theory. In order to form bond the atoms present in the reactants should collide each other for the bond formation.

In order to establish the plausibility of a mechanism, one must compare the rate law of the rate determining step to the experimentally determined rate law.

Rate law: It is generally the rate equation that consists of the reaction rate with the concentration or the pressures of the reactants and constant parameters.

Rate determining step: In a chemical reaction the rate determining step is the slowest step in which the rate of the reaction depends on the rate of that slowest step.

The rate of a reaction is defined by the change in concentration of substrate (reactant) or target (product) with change in time.

  $\begin{array}{c}\text{Rate}\text{=}\frac{\text{Concentration}\text{change}\left(\text{in}\text{reactant}\text{or}\text{product}\right)}{\text{Time}\text{change}}\\ \\ =\left(-\frac{1}{a}.\frac{\Delta \left[A\right]}{\Delta t}\right)=\left(\frac{1}{b}.\frac{\Delta \left[B\right]}{\Delta t}\right)\end{array}$

Rate constant: The rate constant for a chemical reaction is the proportionality term in the chemical reaction rate law which gives the relationship between the rate and the concentration of the reactant present in the chemical reaction.

Rate order: The order of each reactant in a reaction is represented by the exponential term of the respective reactant present in the rate law and the overall order of the reaction is the sum of all the exponents of all reactants present in the chemical reaction. The order of the reaction is directly proportional to the concentration of the reactants.