Chapter 6, Problem 6.66SP

(a)

Interpretation Introduction

Interpretation:

The balanced reaction of preparing pure Oxygen from $\text{HgO}$ has to be identified.

Concept introduction:

Balanced reaction is a chemical reaction in which number of atoms for each element in the reaction and the total charge are same on both reactant side and the product side.

Steps in balancing the information

• Step 1: Write the unbalanced equation
• Step 2: Find the coefficient to balance the equation.

The coefficient should be reduced to the smallest whole number

(b)

Interpretation Introduction

Interpretation:

The number of grams of $\text{Hg}$ and oxygen are needed to form from $\text{45}\text{.5 g}$ of $\text{HgO}$ has to be calculated.

Concept introduction:

Number of moles:

One mole is the equal to number of atoms in $\text{12g}$ of carbon $\text{-12}$ which is equal to $\text{6}{\text{.023×10}}^{\text{23}}$ atoms. This is also known as Avogadro number.

Number of moles can be calculated as:

Number of moles = $\frac{\text{given}\text{mass of the element}}{\text{atomic}\text{mass}\text{of}\text{element}}$

Number of grams = number of moles $\text{×}$ atomic mass of the element

(c)

Interpretation Introduction

Interpretation:

The number of grams of $\text{HgO}$ are needed to form from $\text{33}\text{.3}\text{g}$ of ${\text{O}}_{\text{2}}$ has to be calculated.

Concept introduction:

Number of moles:

One mole is the equal to number of atoms in $\text{12g}$ of carbon $\text{-12}$ which is equal to $\text{6}{\text{.023×10}}^{\text{23}}$ atoms. This is also known as Avogadro number.

Number of moles can be calculated as:

Number of moles = $\frac{\text{given}\text{mass of the element}}{\text{atomic}\text{mass}\text{of}\text{element}}$

Number of grams = number of moles $\text{×}$ atomic mass of the element