Chapter 15, Problem 15.153MP

Interpretation Introduction

(a)

Interpretation:

The value of ${\text{K}}_{\text{p}}$ needs to be determined.

Concept introduction:

At equilibrium, the constant which is used to express the relationship between reactants and products at the given temperature in a reversible chemical heat reaction is known as equilibrium constant.

For a reversible chemical reaction:

$\text{aA+bB}\to \text{cC+dD}$

The equilibrium constant is given by the following expression:

$\text{K=}\frac{{\left[\text{C}\right]}^{\text{c}}\text{.}{\left[\text{D}\right]}^{\text{d}}}{{\left[\text{A}\right]}^{\text{a}}\text{.}{\left[\text{B}\right]}^{\text{b}}}$

Where,

Equilibrium concentration of $\text{A}$ : $\left[\text{A}\right]$

Equilibrium concentration of $\text{B}$ : $\left[\text{B}\right]$

Equilibrium concentration of $\text{C}$ : $\left[\text{C}\right]$

Equilibrium concentration of $\text{D}$ : $\left[\text{D}\right]$

Interpretation Introduction

(b)

Interpretation:

The partial pressure of cyclopropane for the given condition at $\text{500K}$ needs to be determined.

Concept introduction:

A general equilibrium reaction can be written as follows:

$aA+bB\rightleftharpoons cC+dD$

For a general reaction, the expression for K_c can be represented as follows:

$K_c=\frac{{\left[C\right]}^c{\left[D\right]}^d}{{\left[A\right]}^a{\left[B\right]}^b}$

It can also be written in the form of partial pressure of all the gases as follows:

$K_p=\frac{{\left(P_C\right)}^c{\left(P_D\right)}^d}{{\left(P_A\right)}^a{\left(P_B\right)}^b}$

Interpretation Introduction

(c)

Interpretation:

The changes after altering the ratio of the two concentrations at equilibrium needs to be explained by adding cyclopropane or decreasing the volume of a container

Concept introduction:

A general equilibrium reaction can be written as follows:

$aA+bB\rightleftharpoons cC+dD$

For a general reaction, the expression for K_c can be represented as follows:

$K_c=\frac{{\left[C\right]}^c{\left[D\right]}^d}{{\left[A\right]}^a{\left[B\right]}^b}$

It can also be written in the form of partial pressure of all the gases as follows:

$K_p=\frac{{\left(P_C\right)}^c{\left(P_D\right)}^d}{{\left(P_A\right)}^a{\left(P_B\right)}^b}$

Interpretation Introduction

(d)

Interpretation:

The reaction with the larger rate constant out of reverse and forward needs to be determined.

Concept introduction:

A general equilibrium reaction can be written as follows:

$aA+bB\rightleftharpoons cC+dD$

For a general reaction, the expression for K_c can be represented as follows:

$K_c=\frac{{\left[C\right]}^c{\left[D\right]}^d}{{\left[A\right]}^a{\left[B\right]}^b}$

It can also be written in the form of partial pressure of all the gases as follows:

$K_p=\frac{{\left(P_C\right)}^c{\left(P_D\right)}^d}{{\left(P_A\right)}^a{\left(P_B\right)}^b}$

Interpretation Introduction

(e)

Interpretation:

Thereason of reactive cyclopropane needs to be explained.

Concept introduction:

A general equilibrium reaction can be written as follows:

$aA+bB\rightleftharpoons cC+dD$

For a general reaction, the expression for K_c can be represented as follows:

$K_c=\frac{{\left[C\right]}^c{\left[D\right]}^d}{{\left[A\right]}^a{\left[B\right]}^b}$

It can also be written in the form of partial pressure of all the gases as follows:

$K_p=\frac{{\left(P_C\right)}^c{\left(P_D\right)}^d}{{\left(P_A\right)}^a{\left(P_B\right)}^b}$