Chapter 14, Problem 97SCQ

### Chemistry & Chemical Reactivity

10th Edition
John C. Kotz + 3 others
ISBN: 9781337399074

Chapter
Section

### Chemistry & Chemical Reactivity

10th Edition
John C. Kotz + 3 others
ISBN: 9781337399074
Textbook Problem

# The reaction cyclopropane → propene occurs on a platinum metal surface at 200 °C. (The platinum is a catalyst.) The reaction is first-order in cyclopropane. Indicate how the following quantities change (increase, decrease, or no change) as this reaction progresses, assuming constant temperature. (a) [cyclopropane] (b) [propene] (c) [catalyst] (d) the rate constant, k (e) the order of the reaction (f) the half-life of cyclopropane

(a)

Interpretation Introduction

Interpretation:

The change in [cyclopropane] as the reaction proceeds should be determined.

Concept introduction:

Rate law or rate equation: 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.

aA + bBxXRate of reaction = k [A]m[B]n

Explanation

As the given reaction proceed the reactant gets reduced which results in increase in the product as the given reaction is the forward reaction since the arrow used in the given representation tends towards right side direction.

Therefore, the given quantity [<

(b)

Interpretation Introduction

Interpretation:

The change in [propane] as the reaction proceeds should be determined.

Concept introduction:

Rate law or rate equation: 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.

aA + bBxXRate of reaction = k [A]m[B]n

(c)

Interpretation Introduction

Interpretation:

The change in [catalyst] as the reaction proceeds should be determined.

Concept introduction:

Rate law or rate equation: 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.

aA + bBxXRate of reaction = k [A]m[B]n

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.

(d)

Interpretation Introduction

Interpretation:

The change in the rate constant, k as the reaction proceeds should be determined.

Concept introduction:

Rate law or rate equation: 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.

aA + bBxXRate of reaction = k [A]m[B]n

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.

(e)

Interpretation Introduction

Interpretation:

The change in the order of the reaction as the reaction proceeds should be determined.

Concept introduction:

Rate law or rate equation: 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.

aA + bBxXRate of reaction = k [A]m[B]n

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.

(f)

Interpretation Introduction

Interpretation:

The change in the half–life of cyclopropane as the reaction proceeds should be determined.

Concept introduction:

Rate law or rate equation: 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.

aA + bBxXRate of reaction = k [A]m[B]n

Half–lifet1/2: The half–life period is defined as the time required by the reactant to reduce its concentration to one half of its initial concentration.

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