   Chapter 14, Problem 60GQ

Chapter
Section
Textbook Problem

Data in the table were collected at 540 K for the following reaction:CO(g) + NO2(g) → CO2(g) + NO(g) Using the data in the table: (a) Determine the reaction order with respect to each reactant. (b) Derive the rate equation. (c) Calculate the rate constant, giving the correct units for k.

(a)

Interpretation Introduction

Interpretation:

The reaction order with respect to each reactant has to be determined.

Concept introduction:

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

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.

Intermediate species: It is the species formed during the middle of the chemical reaction between the reactant and the desired product.

Molecularity: The molecularity of the reaction actually denotes the number of species that present in the rate determining step of the reaction.

Activation energy: It is 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.

Rate order: It 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.

Explanation

From the given set of concentration and rate data, the order for each reactant present in the reaction is determined as follows:

First, divide the first given rate data with the fourth given data in order to determine the order for CO

[CO]1[CO]4[NO2]1[NO2]4Rate1Rate45.1×1041.0×1030.35×1040.35×104=3.4×1086.8×108(0.51)m=(0.51)1OrderofCO=1

Then, divide the first given rate data with the second given data in order to determine the order for NO2

(b)

Interpretation Introduction

Interpretation:

The rate equation has to be derived.

Concept introduction:

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.

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.

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.

(c)

Interpretation Introduction

Interpretation:

The rate constant for the given reaction has to be calculated by giving the correct units for k

Concept introduction:

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.

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.

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.

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