Chapter 9.4, Problem 9.25QAP

Interpretation Introduction

(a)

Interpretation:

To calculate the amount of SO₃ produced when given amounts of reactants react according to following reaction:

  ${\text{2SO}}_{\text{2}}\text{(g)}\text{+}{\text{O}}_{\text{2}}\text{(g)}\stackrel{}{\to }{\text{2SO}}_{\text{3}}\text{(g)}$

Concept Introduction:

A stoichiometric coefficient of a well-balanced chemical equation tells about the relative relation between moles of reactants used and moles of products formed.

Lets say we have a chemical reaction as:

  $\text{aA}\text{+bB}\to \text{cC}\text{+}\text{dD}$

If above reaction is well-balanced then,

a moles of A reacts with b moles of B to produce c moles of C and d moles of D.

Limiting reactant: It is reactant in a chemical reaction which limits the amounts of products formed.

After complete utilization of limiting reactant, no more products are formed.

Way to determine limiting reactant:

• Calculate moles of each reactant.
• Divide moles of each reactant with their respective stoichiometric coefficient from well-balanced chemical equation.
• Lower value corresponds to the limiting reactant.

Interpretation Introduction

(b)

Interpretation:

To calculate the amount of Fe₃O₄ produced when given amounts of reactants react according to following reaction:

  $\text{3Fe}\text{(s)}\text{+}{\text{4H}}_{\text{2}}\text{O}\text{(l)}\stackrel{}{\to }{\text{Fe}}_3{\text{O}}_4\text{(s)}\text{+}{\text{4H}}_{\text{2}}\text{(g)}$

Concept Introduction:

A stoichiometric coefficient of a well-balanced chemical equation tells about the relative relation between moles of reactants used and moles of products formed.

Lets say we have a chemical reaction as:

  $\text{aA}\text{+bB}\to \text{cC}\text{+}\text{dD}$

If above reaction is well-balanced then,

a moles of A reacts with b moles of B to produce c moles of C and d moles of D.

Limiting reactant: It is reactant in a chemical reaction which limits the amount of products formed.

After complete utilization of limiting reactant, no more products are formed.

Way to determine limiting reactant:

• Calculate moles of each reactant.
• Divide moles of each reactant with their respective stoichiometric coefficient from well-balanced chemical equation.
• Lower value corresponds to the limiting reactant.

Interpretation Introduction

(c)

Interpretation:

To calculate the amount of CO₂ produced when given amounts of reactants react according to following reaction:

  ${\text{C}}_{\text{7}}{\text{H}}_{\text{16}}\text{(l)}\text{+}\text{11}{\text{O}}_{\text{2}}\text{(g)}\stackrel{}{\to }{\text{7CO}}_{\text{2}}\text{(g)}\text{+}{\text{8H}}_{\text{2}}\text{O (g)}$

Concept Introduction:

A stoichiometric coefficient of a well-balanced chemical equation tells about the relative relation between moles of reactants used and moles of products formed.

Lets say we have a chemical reaction as:

  $\text{aA}\text{+bB}\to \text{cC}\text{+}\text{dD}$

If above reaction is well-balanced then,

a moles of A reacts with b moles of B to produce c moles of C and d moles of D.

Limiting reactant: It is reactant in a chemical reaction which limits the amounts of products formed.

After complete utilization of limiting reactant, no more products are formed.

Way to determine limiting reactant:

• Calculate moles of each reactant.
• Divide moles of each reactant with their respective stoichiometric coefficient from well-balanced chemical equation.
• Lower value corresponds to the limiting reactant.