Chapter 10, Problem 10.4P

(a)

Interpretation Introduction

Interpretation:

The species which are present on the surface are to be identified.

Concept Introduction:

The rate law of the chemical reaction states that the rate of reaction is the function of the concentration of the reactants and the products present in that specific reaction. The rate is actually predicted by the slowest step of the reaction.

If there is a chemical reaction which has reactants A and B that reacts to form products then their rate law is given as follows.

    $r=k{\left[A\right]}^a{\left[B\right]}^b$

Here, $\left[A\right]$ is the concentration of the reactant A, $\left[B\right]$ is the concentration of the reactant B and $k$ is the rate constant.

(b)

Interpretation Introduction

Interpretation:

An explanation regarding the reversibility obtained from Figure B is to be stated and the species that adsorbed on the surface are to be identified.

Concept Introduction:

The rate law of the chemical reaction states that the rate of reaction is the function of the concentration of the reactants and the products present in that specific reaction. The rate is actually predicted by the slowest step of the reaction.

If there is a chemical reaction which has reactants A and B that reacts to form products then their rate law is given as follows.

    $r=k{\left[A\right]}^a{\left[B\right]}^b$

Here, $\left[A\right]$ is the concentration of the reactant A, $\left[B\right]$ is the concentration of the reactant B and $k$ is the rate constant.

(c)

Interpretation Introduction

Interpretation:

The rate law and a rate-limiting step that is consistent with the given Figures are to be stated.

Concept Introduction:

The rate law of the chemical reaction states that the rate of reaction is the function of the concentration of the reactants and the products present in that specific reaction. The rate is actually predicted by the slowest step of the reaction.

If there is a chemical reaction which has reactants A and B that reacts to form products then their rate law is given as follows.

    $r=k{\left[A\right]}^a{\left[B\right]}^b$

Here, $\left[A\right]$ is the concentration of the reactant A, $\left[B\right]$ is the concentration of the reactant B and $k$ is the rate constant.

(d)

Interpretation Introduction

Interpretation:

The way by which the plot is obtained to linearize the initial rate data in Figure A is to be stated.

Concept Introduction:

The rate law of the chemical reaction states that the rate of reaction is the function of the concentration of the reactants and the products present in that specific reaction. The rate is actually predicted by the slowest step of the reaction.

If there is a chemical reaction which has reactants A and B that reacts to form products then their rate law is given as follows.

    $r=k{\left[A\right]}^a{\left[B\right]}^b$

Here, $\left[A\right]$ is the concentration of the reactant A, $\left[B\right]$ is the concentration of the reactant B and $k$ is the rate constant.

(e)

Interpretation Introduction

Interpretation:

The conversion at which the number of sites with A adsorbed on the surface and C adsorbed on the surface becomes equal is to be calculated.

Concept Introduction:

The real reactor is defined as the process vessel which is used to perform a chemical reaction. It is modeled by various combinations of ideal reactors. The conversion, X can be defined as the moles of any species A that are reacted per mole of A fed in the reactor.