Chapter 9.1, Problem 4RQ

Interpretation Introduction

Interpretation: The number of moles of ${\text{O}}_2(g)$ required to react with 3.6 mole of ${\text{SO}}_2\text{(g)}$ in the given reaction needs to be calculated.

Concept introduction:The ratio of mass of substance to its molar mass is said to be number of moles of that substance.

The ratio of amount of any two compounds involved in a chemical reaction in terms of mole is said to be mole ratio, and used as a conversion factor between reactants and products.

Answer to Problem 4RQ

The number of moles of ${\text{O}}_2(g)$ required to react with 3.6 mole of ${\text{SO}}_2\text{(g)}$ in the given reaction is $\text{1}\text{.8 mol}$ .

Explanation of Solution

Given:

  ${\text{2SO}}_2(g)+{\text{ O}}_2(g)\to {\text{ 2SO}}_3(g)$

From the balanced chemical reaction, the mole ratio of sulfur dioxide and oxygen is 2:1 so, the number of moles of oxygen required for 3.6 moles of sulfur dioxide is:

  $\text{3}{\text{.6 mol of SO}}_2\text{×}\frac{{\text{1 mol of O}}_{\text{2}}}{{\text{2 mol of SO}}_2}\text{ = 1}{\text{.8 mol of O}}_{\text{2}}$

Hence, the number of moles of ${\text{O}}_2(g)$ required to react with 3.6 mole of ${\text{SO}}_2\text{(g)}$ in the given reaction is $\text{1}\text{.8 mol}$ .