Chapter 3, Problem 3.77P

(a)

Interpretation Introduction

Interpretation:

A balanced equation for each step in the formation of iodine trichloride 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: 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 2: 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. Generally, oxygen atoms are balanced in last.

Step 3: 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. Generally, oxygen atoms are balanced in last.

Step 4: Check whether the chemical equation is balanced or not by counting the number of atoms of each element on both sides.

(b)

Interpretation Introduction

Interpretation:

A balanced equation for the overall formation of iodine trichloride 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: 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 2: 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. Generally, oxygen atoms are balanced in last.

Step 3: 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. Generally, oxygen atoms are balanced in last.

Step 4: Check whether the chemical equation is balanced or not by counting the number of atoms of each element on both sides.

(c)

Interpretation Introduction

Interpretation:

The amount $\left(\text{g}\right)$ of iodine required to form $2.45\text{ kg}$ iodine trichloride is to be determined.

Concept introduction:

The mole ratio from the balanced chemical equation is used for determining the moles of product.

The conversion factor to convert amount in $\text{kg}$ into $\text{g}$ is as follows:

  $\text{Mass}\left(\text{g}\right)=\left(\text{Mass}\left(\text{kg}\right)\right)\left(\frac{{10}^3\text{ g}}{1\text{ kg}}\right)$        (5)