Chapter 3.3, Problem 3.12BFP

(a)

Interpretation Introduction

Interpretation:

A balanced chemical equation for the explosive decomposition of liquid nitroglycerine to form carbon dioxide, water vapor, nitrogen, and oxygen is to be written.

Concept introduction:

In a balanced chemical equation, the total mass of reactants and products are equal in a balanced chemical equation, thus, it obeyed the law of conservation of mass.

Following are the steps to write a balanced chemical equation.

Step 1: Translate the chemical statement into a skeleton equation. The chemical substances that undergo a change are termed as reactants and the chemical substances that are produced during the chemical change are termed as products. The reactants are specified on the left side of the yield arrow while the products are specified on the right side of the yield arrow. Put a blank before each formula while beginning the balancing process.

Step 2: Identify the most complex substance and choose an element such that the element must be present only in one reactant and one product. Place the stoichiometric coefficient before the element(s) such that the number of atoms of that element(s) is the same on both sides.

Step 3: Balance the remaining atoms by placing the stoichiometric coefficients before the element(s) such that the number of atoms of that element(s) is the same on both sides. Identify the least complex substance and end with it.

Step 4: In a balanced chemical reaction, the smallest whole number coefficients are most preferred. Hence, adjusting the coefficients in such a way that the smallest whole number coefficients are obtained for each element.

Step 5: Check whether the chemical equation is balanced or not by counting the number of atoms of each element on both sides.

Step 6: Specify the states of matter of each chemical substance present in the balanced chemical equation. The table for the abbreviations used for each state is as follows:

$\begin{array}{cc}\text{State}& \text{Abbreviation}\\ \text{Solid}& s\\ \text{Liquid}& l\\ \text{Gas}& g\\ \begin{array}{l}\text{Aqueous}\\ \text{solution}\end{array}& aq\end{array}$

(b)

Interpretation Introduction

Interpretation:

A balanced chemical equation for the reaction between solid potassium superoxide and carbon dioxide to form oxygen gas and solid potassium carbonate is to be written.

Concept introduction:

In a balanced chemical equation, the total mass of reactants and products are equal in a balanced chemical equation, thus, it obeyed the law of conservation of mass.

Following are the steps to write a balanced chemical equation.

Step 1: Translate the chemical statement into a skeleton equation. The chemical substances that undergo a change are termed as reactants and the chemical substances that are produced during the chemical change are termed as products. The reactants are specified on the left side of the yield arrow while the products are specified on the right side of the yield arrow. Put a blank before each formula while beginning the balancing process.

Step 2: Identify the most complex substance and choose an element such that the element must be present only in one reactant and one product. Place the stoichiometric coefficient before the element(s) such that the number of atoms of that element(s) is the same on both sides.

Step 3: Balance the remaining atoms by placing the stoichiometric coefficients before the element(s) such that the number of atoms of that element(s) is the same on both sides. Identify the least complex substance and end with it.

Step 4: In a balanced chemical reaction, the smallest whole number coefficients are most preferred. Hence, adjusting the coefficients in such a way that the smallest whole number coefficients are obtained for each element.

Step 5: Check whether the chemical equation is balanced or not by counting the number of atoms of each element on both sides.

Step 6: Specify the states of matter of each chemical substance present in the balanced chemical equation. The table for the abbreviations used for each state is as follows:

$\begin{array}{cc}\text{State}& \text{Abbreviation}\\ \text{Solid}& s\\ \text{Liquid}& l\\ \text{Gas}& g\\ \begin{array}{l}\text{Aqueous}\\ \text{solution}\end{array}& aq\end{array}$

(c)

Interpretation Introduction

Interpretation:

A balanced chemical equation for the reaction in a blast furnace between solid iron(III) oxide and carbon monoxide to form solid iron metal and carbon dioxide gas is to be written.

Concept introduction:

In a balanced chemical equation, the total mass of reactants and products are equal in a balanced chemical equation, thus, it obeyed the law of conservation of mass.

Following are the steps to write a balanced chemical equation.

Step 1: Translate the chemical statement into a skeleton equation. The chemical substances that undergo a change are termed as reactants and the chemical substances that are produced during the chemical change are termed as products. The reactants are specified on the left side of the yield arrow while the products are specified on the right side of the yield arrow. Put a blank before each formula while beginning the balancing process.

Step 2: Identify the most complex substance and choose an element such that the element must be present only in one reactant and one product. Place the stoichiometric coefficient before the element(s) such that the number of atoms of that element(s) is the same on both sides.

Step 3: Balance the remaining atoms by placing the stoichiometric coefficients before the element(s) such that the number of atoms of that element(s) is the same on both sides. Identify the least complex substance and end with it.

Step 4: In a balanced chemical reaction, the smallest whole number coefficients are most preferred. Hence, adjusting the coefficients in such a way that the smallest whole number coefficients are obtained for each element.

Step 5: Check whether the chemical equation is balanced or not by counting the number of atoms of each element on both sides.

Step 6: Specify the states of matter of each chemical substance present in the balanced chemical equation. The table for the abbreviations used for each state is as follows:

$\begin{array}{cc}\text{State}& \text{Abbreviation}\\ \text{Solid}& s\\ \text{Liquid}& l\\ \text{Gas}& g\\ \begin{array}{l}\text{Aqueous}\\ \text{solution}\end{array}& aq\end{array}$