Chapter 14, Problem 92SCQ

Interpretation Introduction

Interpretation:

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

Concept introduction:

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

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

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.

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.

Activation energy: It is defined as the minimum energy required by the reacting species in order to undergo chemical reaction.

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.

Catalyst: The catalyst is a chemical substance that increases the rate of the reaction without participating in the reaction by reducing the activation energy of the reaction.