Ch.4 - Chemical Reactions and Chemical Quantities

Problem 37b

Chapter 4, Problem 37b

Consider the reaction: 4 HCl(g) + O₂(g) → 2 H₂O(g) + 2 Cl₂(g) Each molecular diagram represents an initial mixture of reactants. How many molecules of Cl₂ form from the reaction mixture that produces the greatest amount of products?

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Identify the balanced chemical equation: 4 \text{HCl}(g) + \text{O}_2(g) \rightarrow 2 \text{H}_2\text{O}(g) + 2 \text{Cl}_2(g)

Determine the stoichiometric ratios from the balanced equation: 4 moles of HCl react with 1 mole of O_2 to produce 2 moles of Cl_2.

Examine the initial mixture of reactants to identify the limiting reactant by comparing the available moles of HCl and O_2.

Calculate the maximum number of Cl_2 molecules that can be formed based on the limiting reactant using the stoichiometric ratio.

Verify the calculation by ensuring that the number of Cl_2 molecules formed does not exceed the amount predicted by the stoichiometry of the reaction.

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Key Concepts

Here are the essential concepts you must grasp in order to answer the question correctly.

Stoichiometry

Stoichiometry is the calculation of reactants and products in chemical reactions based on the balanced equation. It allows us to determine the proportions of each substance involved in the reaction, which is essential for predicting how much product will form from given amounts of reactants.

Limiting Reactant

The limiting reactant is the substance that is completely consumed first in a chemical reaction, thus determining the maximum amount of product that can be formed. Identifying the limiting reactant is crucial for calculating the yield of products, as it dictates how far the reaction can proceed.

Molecular Ratios

Molecular ratios are derived from the coefficients of a balanced chemical equation and indicate the relative amounts of reactants and products involved in the reaction. Understanding these ratios is vital for predicting the quantities of products formed from specific amounts of reactants, particularly in determining how many molecules of Cl<sub>2</sub> can be produced.

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Related Practice

Textbook Question

For each of the reactions, calculate the mass (in grams) of the product that forms when 15.39 g of the underlined reactant completely reacts. Assume that there is more than enough of the other reactant.

a. 2 K(s) + Cl₂(g) → 2 KCl(s)

b. 2 K(s) + Br₂(l) → 2 KBr(s)

c. 4 Cr(s) + 3 O₂(g) → 2 Cr₂O₃(s)

d. 2 Sr(s) + O₂(g) → 2 SrO(s)

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Textbook Question

Find the limiting reactant for each initial amount of reactants.

2 Na(s) + Br₂(g) → 2 NaBr(s)

a. 2 mol Na, 2 mol Br₂

b. 1.8 mol Na, 1.4 Br₂

c. 2.5 mol Na, 1 mol Br₂

d. 12.6 mol Na, 6.9 mol Br₂

Find the limiting reactant for each initial amount of reactants. 4 Al(s) + 3 O₂( g) → 2 Al₂O₃(s)

a. 1 mol Al, 1 mol O₂

b. 4 mol Al, 2.6 mol O₂

c. 16 mol Al, 13 mol O₂

d. 7.4 mol Al, 6.5 mol O₂

Consider the reaction: 2 CH₃OH(g) + 3 O₂(g) → 2 CO₂(g) + 4 H₂O(g) Each of the molecular diagrams represents an initial mixture of the reactants. How many CO₂ molecules form from the reaction mixture that produces the greatest amount of products?

Calculate the theoretical yield of the product (in moles) for each initial amount of reactants.

Ti(s) + 2 Cl₂(g) → TiCl₄(s)

a. 4 mol Ti, 4 mol Cl₂

b. 7 mol Ti, 17 mol Cl₂

c. 12.4 mol Ti, 18.8 mol Cl₂

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Textbook Question