Chapter 17, Problem 20A

(a)

Interpretation Introduction

Interpretation: The equilibrium expression for the given reaction has to be written. The given reaction is,

  ${\text{NO}}_{\text{2}}\left(\text{g}\right)\text{+ClNO}\left(\text{g}\right)\to {\text{ClNO}}_{\text{2}}\left(\text{g}\right)\text{+NO}\left(\text{g}\right)$

Concept Introduction: For a balanced chemical reaction,

  $aA+bB\rightleftharpoons cC+dD$

The equilibrium expression is the ratio of the concentration of the products to the concentration of the reaction. The concentration of each reactant/product is raised to a power corresponding to their coefficient in the balanced equation.

The law of chemical equilibrium is given by the equilibrium expression,

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

The equilibrium constant is represented as $K.$

Answer to Problem 20A

The equilibrium expression for the reaction is $K=\frac{\left[{\text{ClNO}}_{\text{2}}\right]\left[\text{NO}\right]}{\left[{\text{NO}}_{\text{2}}\right]\left[\text{ClNO}\right]}\text{.}$

Explanation of Solution

The given reaction is,

  ${\text{NO}}_{\text{2}}\left(\text{g}\right)\text{+ClNO}\left(\text{g}\right)\to {\text{ClNO}}_{\text{2}}\left(\text{g}\right)\text{+NO}\left(\text{g}\right)$

For a balanced chemical reaction,

  $aA+bB\rightleftharpoons cC+dD$

The equilibrium expression is the ratio of the concentration of the products to the concentration of the reaction. The concentration of each reactant/product is raised to a power corresponding to their coefficient in the balanced equation.

Where,

• $A,B,C,D$ are chemical species.
• $a,b,c$ and $d$ are coefficients in the balanced equation.

The law of chemical equilibrium is given by the equilibrium expression,

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

The equilibrium constant is represented as $K.$

For the given reaction, the equilibrium expression is written as,

  $K=\frac{\left[{\text{ClNO}}_{\text{2}}\right]\left[\text{NO}\right]}{\left[{\text{NO}}_{\text{2}}\right]\left[\text{ClNO}\right]}$

The equilibrium expression for the reaction is $K=\frac{\left[{\text{ClNO}}_{\text{2}}\right]\left[\text{NO}\right]}{\left[{\text{NO}}_{\text{2}}\right]\left[\text{ClNO}\right]}\text{.}$

(b)

Interpretation Introduction

Interpretation: The equilibrium expression for the given reaction has to be written. The given reaction is,

  ${\text{Br}}_{\text{2}}\left(\text{g}\right){\text{+5F}}_{\text{2}}\left(\text{g}\right)\rightleftharpoons {\text{2BrF}}_{\text{5}}\left(\text{g}\right)$

Concept Introduction: For a balanced chemical reaction,

  $aA+bB\rightleftharpoons cC+dD$

The equilibrium expression is the ratio of the concentration of the products to the concentration of the reaction. The concentration of each reactant/product is raised to a power corresponding to their coefficient in the balanced equation.

The law of chemical equilibrium is given by the equilibrium expression,

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

The equilibrium constant is represented as $K.$

Answer to Problem 20A

The equilibrium expression for the reaction is $K=\frac{{\left[{\text{BrF}}_{\text{5}}\right]}^{\text{2}}}{\left[{\text{Br}}_{\text{2}}\right]{\left[{\text{F}}_{\text{2}}\right]}^{\text{5}}}\text{.}$

Explanation of Solution

The given reaction is,

  ${\text{Br}}_{\text{2}}\left(\text{g}\right){\text{+5F}}_{\text{2}}\left(\text{g}\right)\rightleftharpoons {\text{2BrF}}_{\text{5}}\left(\text{g}\right)$

For a balanced chemical reaction,

  $aA+bB\rightleftharpoons cC+dD$

The equilibrium expression is the ratio of the concentration of the products to the concentration of the reaction. The concentration of each reactant/product is raised to a power corresponding to their coefficient in the balanced equation.

Where,

• $A,B,C,D$ are chemical species.
• $a,b,c$ and $d$ are coefficients in the balanced equation.

The law of chemical equilibrium is given by the equilibrium expression,

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

The equilibrium constant is represented as $K.$

For the given reaction, the equilibrium expression is written as,

  $K=\frac{{\left[{\text{BrF}}_{\text{5}}\right]}^{\text{2}}}{\left[{\text{Br}}_{\text{2}}\right]{\left[{\text{F}}_{\text{2}}\right]}^{\text{5}}}$

The equilibrium expression for the reaction is $K=\frac{{\left[{\text{BrF}}_{\text{5}}\right]}^{\text{2}}}{\left[{\text{Br}}_{\text{2}}\right]{\left[{\text{F}}_{\text{2}}\right]}^{\text{5}}}\text{.}$

(c)

Interpretation Introduction

Interpretation: The equilibrium expression for the given reaction has to be written. The given reaction is,

  ${\text{4NH}}_{\text{3}}\left(\text{g}\right)\text{+5NO}\left(\text{g}\right)\rightleftharpoons {\text{5N}}_{\text{2}}\left(\text{g}\right){\text{+6H}}_{\text{2}}\text{O}\left(\text{g}\right)$

Concept introduction: For a balanced chemical reaction,

  $aA+bB\rightleftharpoons cC+dD$

The equilibrium expression is the ratio of the concentration of the products to the concentration of the reaction. The concentration of each reactant/product is raised to a power corresponding to their coefficient in the balanced equation.

The law of chemical equilibrium is given by the equilibrium expression,

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

The equilibrium constant is represented as $K.$

Answer to Problem 20A

The equilibrium expression for the reaction is $K=\frac{{\left[{\text{N}}_{\text{2}}\right]}^{\text{5}}{\left[{\text{H}}_{\text{2}}\text{O}\right]}^{\text{6}}}{{\left[{\text{NH}}_{\text{3}}\right]}^{\text{4}}{\left[\text{NO}\right]}^{\text{6}}}\text{.}$

Explanation of Solution

The given reaction is,

  ${\text{4NH}}_{\text{3}}\left(\text{g}\right)\text{+5NO}\left(\text{g}\right)\rightleftharpoons {\text{5N}}_{\text{2}}\left(\text{g}\right){\text{+6H}}_{\text{2}}\text{O}\left(\text{g}\right)$

For a balanced chemical reaction,

  $aA+bB\rightleftharpoons cC+dD$

The equilibrium expression is the ratio of the concentration of the products to the concentration of the reaction. The concentration of each reactant/product is raised to a power corresponding to their coefficient in the balanced equation.

Where,

• $A,B,C,D$ are chemical species.
• $a,b,c$ and $d$ are coefficients in the balanced equation.

The law of chemical equilibrium is given by the equilibrium expression,

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

The equilibrium constant is represented as $K.$

For the given reaction, the equilibrium expression is written as,

  $K=\frac{{\left[{\text{N}}_{\text{2}}\right]}^{\text{5}}{\left[{\text{H}}_{\text{2}}\text{O}\right]}^{\text{6}}}{{\left[{\text{NH}}_{\text{3}}\right]}^{\text{4}}{\left[\text{NO}\right]}^{\text{6}}}$

The equilibrium expression for the reaction is $K=\frac{{\left[{\text{N}}_{\text{2}}\right]}^{\text{5}}{\left[{\text{H}}_{\text{2}}\text{O}\right]}^{\text{6}}}{{\left[{\text{NH}}_{\text{3}}\right]}^{\text{4}}{\left[\text{NO}\right]}^{\text{6}}}\text{.}$