Chapter 4, Problem 4.3P

(a)

Interpretation Introduction

Interpretation:

The equilibrium constant $(Kc)$ has to be calculate given elementary of reversible reaction.

Concept Information:

Forward Reaction: This type of reaction has involved irreversible, if obtained product cannot be converted back in to respective reactants under the same conditions.   Backward Reaction: This type of reaction process involved a reversible, if the products can be converted into a back to reactants.

Equilibrium constant: Concentration of the products to the respective molar concentration of reactants it is called equilibrium constant. If the K value is less than one the reaction will move to the left side and the K values is higher (or) greater than one the reaction will move to the right side of reaction.

Rate equation for the general reaction $\text{A+B}\to \text{Product}$ is,

$Rate=\underset{\begin{array}{l}rate\\ constat\end{array}}{k}\left[A\right]\left[B\right]$

The rate of the reaction is proportinal to the concentration of A to the power of x, is ${\left[A\right]}^x$.

The rate of the reaction is proportional to the concentration of B to the power of y is ${\left[B\right]}^y$

Then the rate equation becomes,

$Rate=k{\left[A\right]}^x{\left[B\right]}^y$

Reversible Reaction and equilibrium conversion: The equilibrium, the concentration of the species is related by the relationship dictated by thermodynamic equation.

  $Kc=\frac{C_B^2}{C_A}$

(b)

Interpretation Introduction

Interpretation:

The equilibrium constant value should be determined given liquid-phase reaction.

Concept Information:

Forward Reaction: This type of reaction has involved irreversible, if obtained product cannot be converted back in to respective reactants under the same conditions.   Backward Reaction: This type of reaction process involved a reversible, if the products can be converted into a back to reactants.

Equilibrium constant: Concentration of the products to the respective molar concentration of reactants it is called equilibrium constant. If the K value is less than one the reaction will move to the left side and the K values is higher (or) greater than one the reaction will move to the right side of reaction.

Rate equation for the general reaction $\text{A+B}\to \text{Product}$ is,

$Rate=\underset{\begin{array}{l}rate\\ constat\end{array}}{k}\left[A\right]\left[B\right]$

The rate of the reaction is proportinal to the concentration of A to the power of x, is ${\left[A\right]}^x$.

The rate of the reaction is proportional to the concentration of B to the power of y is ${\left[B\right]}^y$

Then the rate equation becomes,

$Rate=k{\left[A\right]}^x{\left[B\right]}^y$

(c)

Interpretation Introduction

Interpretation:

Equilibrium constant for the given reaction has to be written as a function of conversion, numerically evaluating all possible symbols.

Concept Information:

Rate of a reaction: It represents the speed at which a chemical reaction runs.  How much concentration of substrates (reactants) consumed and how much concentration of targets (products) formed in a unit of time is said to be rate of reaction.

Rate equation for the general reaction $\text{A+B}\to \text{Product}$ is,

$Rate=\underset{\begin{array}{l}rate\\ constat\end{array}}{k}\left[A\right]\left[B\right]$

The rate of the reaction is proportinal to the concentration of A to the power of x, is ${\left[A\right]}^x$.

The rate of the reaction is proportional to the concentration of B to the power of y is ${\left[B\right]}^y$

Then the rate equation becomes,

$Rate=k{\left[A\right]}^x{\left[B\right]}^y$

(d)

Interpretation Introduction

Interpretation:

Equilibrium constant for the given reaction has to be written as a function of conversion, numerically evaluating all possible symbols.

Concept Information:

Rate of a reaction: It represents the speed at which a chemical reaction runs.  How much concentration of substrates (reactants) consumed and how much concentration of targets (products) formed in a unit of time is said to be rate of reaction.

Rate equation for the general reaction $\text{A+B}\to \text{Product}$ is,

$Rate=\underset{\begin{array}{l}rate\\ constat\end{array}}{k}\left[A\right]\left[B\right]$

The rate of the reaction is proportinal to the concentration of A to the power of x, is ${\left[A\right]}^x$.

The rate of the reaction is proportional to the concentration of B to the power of y is ${\left[B\right]}^y$

Then the rate equation becomes,

$Rate=k{\left[A\right]}^x{\left[B\right]}^y$