Chapter 9.4, Problem 9.23QAP

Interpretation Introduction

(a)

Interpretation:To determine the limiting reactant in the following reaction if 20.0 g of each reactant is present initially and calculate the amount of AlCl₃ produced.

  $\text{2Al(s)}\text{+}{\text{3Cl}}_{\text{2}}\text{(g)}\stackrel{}{\to }{\text{2AlCl}}_{\text{3}}\text{(s)}$

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

(b)

Interpretation:To determine the limiting reactant in the following reaction if 20.0 g of each reactant is present initially and calculate the amount of H₂O produced.

  ${\text{4NH}}_{\text{3}}\text{(g)}\text{+}{\text{5O}}_{\text{2}}\text{(g)}\stackrel{}{\to }\text{4NO}\text{(g)}\text{+}{\text{6H}}_{\text{2}}\text{O (g)}$

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 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 determine the limiting reactant in the following reaction if 20.0 g of each reactant is present initially and calculate the amount of SO₂ produced.

  ${\text{CS}}_2\text{(g)}\text{+}3{\text{O}}_{\text{2}}\text{(g)}\stackrel{}{\to }C{\text{O}}_{\text{2}}\text{(g)}\text{+}2S{O}_{\text{2}}\text{ (g)}$

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.