Chapter U4.73, Problem 3E

(a)

Interpretation Introduction

Interpretation:

The given reaction should be classified as single exchange, double exchange, decomposition, and combination reaction and complete the missing product.

  $\text{NaOH}\left(aq\right)+{\text{HNO}}_3\left(aq\right)\to {\text{NaNO}}_{\text{3}}\left(aq\right)+\_\_\_\_\_\_\_\left(l\right)$

Concept Introduction:

The formation of a new compound by the mixing of two or more elements together is termed as combination reaction.

The reaction through which the compound decomposes into one, twosimpler and more than two simplercompounds or elements is known as decomposition reaction. A reaction in whichthe highly or morereactive element replacesa less reactive element is termed as displacement reaction.

Answer to Problem 3E

The given reaction is a double exchange reaction. The complete balanced reaction for it is represented as follows:

  $\text{NaOH}\left(aq\right)+{\text{HNO}}_3\left(aq\right)\to {\text{NaNO}}_{\text{3}}\left(aq\right)+\underset{\_}{{\text{H}}_{\text{2}}\text{O}}\left(l\right)$

Explanation of Solution

The given reaction is represented as follows:

  $\text{NaOH}\left(aq\right)+{\text{HNO}}_3\left(aq\right)\to {\text{NaNO}}_{\text{3}}\left(aq\right)+\_\_\_\_\_\_\_\left(l\right)$

According to the reaction, the exchange or replacement of two elements is taking place that is H, and NO₃ thus, the given reaction is classified as the double exchange reaction. Therefore, the complete reaction is represented as follows:

  $\text{NaOH}\left(aq\right)+{\text{HNO}}_3\left(aq\right)\to {\text{NaNO}}_{\text{3}}\left(aq\right)+\underset{\_}{{\text{H}}_{\text{2}}\text{O}}\left(l\right)$

As the number of elements on the reactant side and product sides are equal thus, the balanced chemical equation for the same is given as follows:

  $\text{NaOH}\left(aq\right)+{\text{HNO}}_3\left(aq\right)\to {\text{NaNO}}_{\text{3}}\left(aq\right)+\underset{\_}{{\text{H}}_{\text{2}}\text{O}}\left(l\right)$

(b)

Interpretation Introduction

Interpretation:

The given reaction should be classified as single exchange, double exchange, decomposition, and combination reaction and complete the missing product.

  ${\text{C}}_{\text{2}}{\text{H}}_{\text{4}}\left(g\right)+{\text{Cl}}_{\text{2}}\left(g\right)\to \_\_\_\_\_\_\_\left(g\right)$

Concept Introduction:

The formation of a new compound by the mixing of two or more elements together is termed as combination reaction.

The reaction through which the compound decomposes into one, twosimpler and more than two simplercompounds or elements is known as decomposition reaction. A reaction in which the highly or more reactive element replaces a less reactive element is termed as displacement reaction.

Answer to Problem 3E

The given reaction is a combination reaction. The complete balanced reaction for it is represented as follows:

  ${\text{C}}_{\text{2}}{\text{H}}_{\text{4}}\left(g\right)+{\text{Cl}}_{\text{2}}\left(g\right)\to \underset{\_}{{\text{C}}_{\text{2}}{\text{H}}_{\text{4}}{\text{Cl}}_{\text{2}}}\left(g\right)$

Explanation of Solution

The given reaction is represented as follows:

  ${\text{C}}_{\text{2}}{\text{H}}_{\text{4}}\left(g\right)+{\text{Cl}}_{\text{2}}\left(g\right)\to \_\_\_\_\_\_\_\left(g\right)$

According to the given reaction, C₂H₄ and Cl₂ reacts with each other to form a single product that means the reaction is a combination reaction. Thus, the complete reaction for it is given as follows:

  ${\text{C}}_{\text{2}}{\text{H}}_{\text{4}}\left(g\right)+{\text{Cl}}_{\text{2}}\left(g\right)\to \underset{\_}{{\text{C}}_{\text{2}}{\text{H}}_{\text{4}}{\text{Cl}}_{\text{2}}}\left(g\right)$

As the number of elements on the reactant side and product sides are equal thus, the balanced chemical equation for the same is given as follows:

  ${\text{C}}_{\text{2}}{\text{H}}_{\text{4}}\left(g\right)+{\text{Cl}}_{\text{2}}\left(g\right)\to \underset{\_}{{\text{C}}_{\text{2}}{\text{H}}_{\text{4}}{\text{Cl}}_{\text{2}}}\left(g\right)$

(c)

Interpretation Introduction

Interpretation:

The given reaction should be classified as single exchange, double exchange, decomposition, and combination reaction and complete the missing product.

  ${\text{Cl}}_{\text{2}}\left(g\right)+{\text{MgBr}}_2\left(s\right)\to {\text{Br}}_2\left(g\right)+\_\_\_\_\_\_\left(s\right)$

Concept Introduction:

The formation of a new compound by the mixing of two or more elements together is termed as combination reaction.

The reaction through which the compound decomposes into one, two simpler and more than two simplercompounds or elements is known as decomposition reaction. A reaction in which the highly or more reactive element replaces a less reactive element is termed as displacement reaction.

Answer to Problem 3E

The given reaction is a single exchange reaction. The complete balanced reaction for it is represented as follows:

  ${\text{Cl}}_{\text{2}}\left(g\right)+{\text{MgBr}}_2\left(s\right)\to {\text{Br}}_2\left(g\right)+\underset{\_}{{\text{MgCl}}_2}\left(s\right)$

Explanation of Solution

The given reaction is represented as follows:

  ${\text{Cl}}_{\text{2}}\left(g\right)+{\text{MgBr}}_2\left(s\right)\to {\text{Br}}_2\left(g\right)+\_\_\_\_\_\_\left(s\right)$

According to the reaction, the exchange or replacement of a single element is taking place that is bromide ion thus, the given reaction is classified as the single exchange reaction. Therefore, the complete reaction is represented as follows:

  ${\text{Cl}}_{\text{2}}\left(g\right)+{\text{MgBr}}_2\left(s\right)\to {\text{Br}}_2\left(g\right)+\underset{\_}{{\text{MgCl}}_2}\left(s\right)$

As the number of elements on the reactant side and product sides are equal thus, the balanced chemical equation for the same is given as follows:

  ${\text{Cl}}_{\text{2}}\left(g\right)+{\text{MgBr}}_2\left(s\right)\to {\text{Br}}_2\left(g\right)+\underset{\_}{{\text{MgCl}}_2}\left(s\right)$