Chapter U4.24, Problem 5E

(a)

Interpretation Introduction

Interpretation:

The moles of NaCl required for the reaction to occur with AgNO₃ should be predicted.

Concept Introduction:

A chemical reaction in which the number of elements on both the reactant and product side is equal and the charge is also equal is known as balanced chemical equation.

The amount of the substance that contains the same number of particles or atoms or molecules is termed as mole.

Answer to Problem 5E

0.10 mol of NaCl are required to react with silver nitrate.

Explanation of Solution

According to the balanced chemical reaction,

  $\begin{array}{c}1\text{mol}{\text{AgNO}}_{\text{3}}\to \text{1}\text{mol}\text{NaCl}\\ \text{0}\text{.10}\text{mol}{\text{AgNO}}_{\text{3}}\to 0.10\text{mol}\text{NaCl}\end{array}$

Thus, 0.10 mol of NaCl are required to react with 0.10 mol of silver nitrate.

(b)

Interpretation Introduction

Interpretation:

The amount of NaCl is grams should be predicted.

Concept Introduction:

The amount of the substance that contains the same number of particles or atoms or molecules is termed as mole.

Answer to Problem 5E

0.10 mol represents 5.844 g NaCl.

Explanation of Solution

Mole can be expressed as the ratio of given mass and molar mass of the compound. The expression for mole is represented as follows:

  $\text{Mole}=\frac{\text{Given}\text{mass}}{\text{Molar}\text{mass}}$

Thus, the mass of NaCl would be calculated as follows:

  $\begin{array}{c}\text{Moles}\text{of}\text{NaCl}=\frac{\text{Given}\text{mass}\text{of}\text{NaCl}}{\text{Molar}\text{mass}\text{of}\text{NaCl}}\\ \text{Given}\text{mass}\text{of}\text{NaCl}=\text{Moles}\text{of}\text{NaCl}\times \text{Molar}\text{mass}\text{of}\text{NaCl}\\ =0.10\text{mol}\times 58.44\text{g/mol}\\ \text{Given}\text{mass}\text{of}\text{NaCl}=5.844\text{g}\end{array}$

Therefore, 0.10 mol represents 5.844 g NaCl.