MCGRAW: CHEMISTRY THE MOLECULAR NATURE
MCGRAW: CHEMISTRY THE MOLECULAR NATURE
8th Edition
ISBN: 9781264330430
Author: VALUE EDITION
Publisher: MCG
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Chapter 4, Problem 4.115P

(a)

Interpretation Introduction

Interpretation:

The reactant present in excess when 1.62 g of lithium is mixed with 6.50 g of oxygen is to be identified.

Concept introduction:

The redox reaction can be classified into three types depending upon the number of reactants and products as follows:

1. Combination redox reaction

2. Decomposition redox reaction

3. Displacement redox reactions

Combination redox reactions are the reactions in which two or more reactants combine to form a single product. In displacement redox reactions, substances on both sides of the equation remain the same but the atoms exchange places in order to form the product while in decomposition reaction, one compound decompose to form one or more product.

A limiting reagent is the one that is completely consumed in a chemical reaction. The amount of product formed in any chemical reaction has to be in accordance with the limiting reagent of the reaction. The amount of product depends on the amount of limiting reagent since the product formation is not possible in the absence of it.

(a)

Expert Solution
Check Mark

Answer to Problem 4.115P

The reactant present in excess when 1.62 g of lithium is mixed with 6.50 g of oxygen is O2.

Explanation of Solution

Lithium combines with oxygen molecule to form lithium oxide (Li2O). The balanced chemical equation of the redox reaction is:

4Li(s)+O2(g)2Li2O(s)

Four moles of Li combine with one mole of O2 to give two mole of Li2O.

The molecular mass of Li is 6.941g/mol.

The formula to calculate moles of Li2O when Li is limiting reagent is:

MolesofLi2O=[(mass ofLi(g)molecular massofLi(g/mol))(2molLi2O4molLi)]                        (1)

Substitute 1.62 g for mass of Li and 6.941g/mol for molecular mass of Li in the equation (1).

MolesofLi2O=[(1.62 g6.941g/mol)(2molLi2O4molLi)]=[(0.23339mol)(2molLi2O4molLi)]=0.1166979mol

The molecular mass of O2 is 32.00g/mol.

The formula to calculate moles of Li2O when O2 is limiting reagent is:

MolesofLi2O=[(mass ofO2(g)molecular massofO2(g/mol))(2molLi2O1molO2)]                       (2)

Substitute 6.50 g for mass of O2 and 32.00g/mol for molecular mass of O2 in the equation (2).

MolesofLi2O=[(6.50 g32.00g/mol)(2molLi2O1molO2)]=[(0.203125mol)(2molLi2O1molO2)]=0.40625mol

Li is limiting reagent in the reaction as the moles of Li2O produced is less in this case as compared to when O2 is the limiting agent.

The reactant present in excess concentration in reaction is O2.

Conclusion

The reactant present in excess when 1.62 g of lithium is mixed with 6.50 g of oxygen is O2.

(b)

Interpretation Introduction

Interpretation:

The moles of product formed when 1.62 g of lithium is mixed with 6.50 g of oxygen is to be calculated.

Concept introduction:

The redox reaction can be classified into three types depending upon the number of reactants and products as follows:

1. Combination redox reaction

2. Decomposition redox reaction

3. Displacement redox reactions

Combination redox reactions are the reactions in which two or more reactants combine to form a single product. In displacement redox reactions, substances on both sides of the equation remain the same but the atoms exchange places in order to form the product while in decomposition reaction, one compound decompose to form one or more product.

A limiting reagent is the one that is completely consumed in a chemical reaction. The amount of product formed in any chemical reaction has to be in accordance with the limiting reagent of the reaction. The amount of product depends on the amount of limiting reagent since the product formation is not possible in the absence of it.

(b)

Expert Solution
Check Mark

Answer to Problem 4.115P

The moles of product formed when 1.62 g of lithium is mixed with 6.50 g of oxygen is 0.1166979mol.

Explanation of Solution

Lithium combines with oxygen molecule to form lithium oxide (Li2O). The balanced chemical equation of the redox reaction is:

4Li(s)+O2(g)2Li2O(s)

Lithium is the limiting agent in the reaction.

Four moles of Li combine with one mole of O2 to give two mole of Li2O.

The molecular mass of Li is 6.941g/mol.

The formula to calculate moles of Li2O when Li is limiting reagent is:

MolesofLi2O=[(mass ofLi(g)molecular massofLi(g/mol))(2molLi2O4molLi)]                        (1)

Substitute 1.62 g for mass of Li and 6.941g/mol for molecular mass of Li in the equation (1).

MolesofLi2O=[(1.62 g6.941g/mol)(2molLi2O4molLi)]=[(0.23339mol)(2molLi2O4molLi)]=0.1166979mol

Conclusion

The moles of product formed when 1.62 g of lithium is mixed with 6.50 g of oxygen is 0.1166979mol.

(c)

Interpretation Introduction

Interpretation:

The mass of each reactant and product after the reaction is to be calculated.

Concept introduction:

The redox reaction can be classified into three types depending upon the number of reactants and products as follows:

1. Combination redox reaction

2. Decomposition redox reaction

3. Displacement redox reactions

Combination redox reactions are the reactions in which two or more reactants combine to form a single product. In displacement redox reactions, substances on both sides of the equation remain the same but the atoms exchange places in order to form the product while in decomposition reaction, one compound decompose to form one or more product.

A limiting reagent is the one that is completely consumed in a chemical reaction. The amount of product formed in any chemical reaction has to be in accordance with the limiting reagent of the reaction. The amount of product depends on the amount of limiting reagent since the product formation is not possible in the absence of it.

(c)

Expert Solution
Check Mark

Answer to Problem 4.115P

The mass of Li, O2 and Li2O after the reaction are 0, 4.63g and 3.49g respectively.

Explanation of Solution

Lithium is the limiting agent in the reaction. Hence, no moles of lithium will left after the completion of reaction.

The molecular mass of Li2O is 29.88g/mol.

The formula to calculate mass of Li2O is:

MassofLi2O=[(moles ofLi2O(mol))(molecularmassofLi2O(g/mol))]          (3)

Substitute 0.1166979mol for moles of Li2O and 29.88g/mol for molecular mass of Li2O in the equation (3).

MassofLi2O=[(0.1166979mol)(29.88g/mol)]=3.4869g3.49g

The formula to calculate mass of O2 reacted is:

MassofO2reacted=[(mass ofLi(g)molecularmassofLi(g/mol))(1molO24molLi)molecularmassofO2(g/mol)]                     (4)

Substitute 1.62 g for mass of Li, 6.941g/mol for molecular mass of Li and 32.00g/mol for molecular mass of O2 in the equation (4).

MassofO2reacted=[(1.62 g6.941g/mol)(1molO24molLi)(32.00g/mol)]=1.867166g

The formula to calculate mass of remaining O2 is:

Remaining O2=(Initial amount ofO2)(Reacted amount ofO2) (5)

Substitute 6.50 g for initial mass of O2 and 1.867166g for reacted mass of O2 in the equation (5).

Remaining O2=(6.50 g)(1.867166g)=4.632834g4.63g

Conclusion

The mass of Li, O2 and Li2O after the reaction are 0, 4.63g and 3.49g respectively.

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Chapter 4 Solutions

MCGRAW: CHEMISTRY THE MOLECULAR NATURE

Ch. 4.1 - A chemist dilutes 60.0 mL of 4.50 M potassium...Ch. 4.1 - Prob. 4.6BFPCh. 4.1 - Prob. 4.7AFPCh. 4.1 - Prob. 4.7BFPCh. 4.3 - Prob. 4.8AFPCh. 4.3 - Prob. 4.8BFPCh. 4.3 - Prob. 4.9AFPCh. 4.3 - Molecular views of the reactant solutions for a...Ch. 4.3 - It is desirable to remove calcium ion from hard...Ch. 4.3 - To lift fingerprints from a crime scene, a...Ch. 4.3 - Despite the toxicity of lead, many of its...Ch. 4.3 - Mercury and its compounds have uses from fillings...Ch. 4.4 - How many OH−(aq) ions are present in 451 mL of...Ch. 4.4 - Prob. 4.12BFPCh. 4.4 - Prob. 4.13AFPCh. 4.4 - Prob. 4.13BFPCh. 4.4 - Prob. 4.14AFPCh. 4.4 - Prob. 4.14BFPCh. 4.4 - Another active ingredient in some antacids is...Ch. 4.4 - Prob. 4.15BFPCh. 4.4 - What volume of 0.1292 M Ba(OH)2 would neutralize...Ch. 4.4 - Calculate the molarity of a solution of KOH if...Ch. 4.5 - Prob. 4.17AFPCh. 4.5 - Prob. 4.17BFPCh. 4.5 - Prob. 4.18AFPCh. 4.5 - Prob. 4.18BFPCh. 4.5 - Prob. 4.19AFPCh. 4.5 - Prob. 4.19BFPCh. 4.6 - Prob. 4.20AFPCh. 4.6 - Prob. 4.20BFPCh. 4 - Prob. 4.1PCh. 4 - What types of substances are most likely to be...Ch. 4 - Prob. 4.3PCh. 4 - Prob. 4.4PCh. 4 - Which of the following scenes best represents how...Ch. 4 - Prob. 4.6PCh. 4 - Prob. 4.7PCh. 4 - Prob. 4.8PCh. 4 - Prob. 4.9PCh. 4 - Prob. 4.10PCh. 4 - A mathematical equation useful for dilution...Ch. 4 - Prob. 4.12PCh. 4 - Prob. 4.13PCh. 4 - Prob. 4.14PCh. 4 - Prob. 4.15PCh. 4 - Does an aqueous solution of each of the following...Ch. 4 - Prob. 4.17PCh. 4 - Prob. 4.18PCh. 4 - Prob. 4.19PCh. 4 - Prob. 4.20PCh. 4 - Prob. 4.21PCh. 4 - Calculate each of the following quantities: Mass...Ch. 4 - Prob. 4.23PCh. 4 - Prob. 4.24PCh. 4 - Prob. 4.25PCh. 4 - Prob. 4.26PCh. 4 - Prob. 4.27PCh. 4 - Prob. 4.28PCh. 4 - Calculate each of the following quantities: Volume...Ch. 4 - Prob. 4.30PCh. 4 - Concentrated sulfuric acid (18.3 M) has a density...Ch. 4 - Prob. 4.32PCh. 4 - Muriatic acid, an industrial grade of concentrated...Ch. 4 - Prob. 4.34PCh. 4 - Prob. 4.35PCh. 4 - Prob. 4.36PCh. 4 - Write two sets of equations (both molecular and...Ch. 4 - Why do some pairs of ions precipitate and others...Ch. 4 - Use Table 4.1 to determine which of the following...Ch. 4 - The beakers represent the aqueous reaction of...Ch. 4 - Complete the following precipitation reactions...Ch. 4 - Prob. 4.42PCh. 4 - Prob. 4.43PCh. 4 - Prob. 4.44PCh. 4 - Prob. 4.45PCh. 4 - Prob. 4.46PCh. 4 - Prob. 4.47PCh. 4 - If 25.0 mL of silver nitrate solution reacts with...Ch. 4 - Prob. 4.49PCh. 4 - Prob. 4.50PCh. 4 - With ions shown as spheres and solvent molecules...Ch. 4 - The precipitation reaction between 25.0 mL of a...Ch. 4 - A 1.50-g sample of an unknown alkali-metal...Ch. 4 - Prob. 4.54PCh. 4 - The mass percent of Cl− in a seawater sample is...Ch. 4 - Prob. 4.56PCh. 4 - Prob. 4.57PCh. 4 - Write a general equation for a neutralization...Ch. 4 - Prob. 4.59PCh. 4 - (a) Name three common weak acids. (b) Name one...Ch. 4 - Prob. 4.61PCh. 4 - Prob. 4.62PCh. 4 - How many moles of H+ ions are present in each of...Ch. 4 - Prob. 4.64PCh. 4 - Prob. 4.65PCh. 4 - Complete the following acid-base reactions with...Ch. 4 - Limestone (calcium carbonate) is insoluble in...Ch. 4 - Prob. 4.68PCh. 4 - Prob. 4.69PCh. 4 - How many grams of NaH2PO4 are needed to react with...Ch. 4 - Prob. 4.71PCh. 4 - Prob. 4.72PCh. 4 - Prob. 4.73PCh. 4 - Prob. 4.74PCh. 4 - Prob. 4.75PCh. 4 - Prob. 4.76PCh. 4 - A mixture of bases can sometimes be the active...Ch. 4 - Describe how to determine the oxidation number of...Ch. 4 - Prob. 4.79PCh. 4 - Prob. 4.80PCh. 4 - Why must every redox reaction involve an oxidizing...Ch. 4 - Prob. 4.82PCh. 4 - Identify the oxidizing agent and the reducing...Ch. 4 - Give the oxidation number of carbon in each of the...Ch. 4 - Prob. 4.85PCh. 4 - Give the oxidation number of nitrogen in each of...Ch. 4 - Give the oxidation number of sulfur in each of the...Ch. 4 - Prob. 4.88PCh. 4 - Give the oxidation number of phosphorus in each of...Ch. 4 - Give the oxidation number of manganese in each of...Ch. 4 - Give the oxidation number of chromium in each of...Ch. 4 - Identify the oxidizing and reducing agents in the...Ch. 4 - Identify the oxidizing and reducing agents in the...Ch. 4 - Identify the oxidizing and reducing agents in the...Ch. 4 - Identify the oxidizing and reducing agents in the...Ch. 4 - The active agent in many hair bleaches is hydrogen...Ch. 4 - A person’s blood alcohol (C2H5OH) level can be...Ch. 4 - Which type of redox reaction leads to each of the...Ch. 4 - Why do decomposition redox reactions typically...Ch. 4 - Which of the types of reactions discussed in...Ch. 4 - Are all combustion reactions redox reactions?...Ch. 4 - Give one example of a combination reaction that is...Ch. 4 - Prob. 4.103PCh. 4 - Prob. 4.104PCh. 4 - Prob. 4.105PCh. 4 - Prob. 4.106PCh. 4 - Prob. 4.107PCh. 4 - Predict the product(s) and write a balanced...Ch. 4 - Prob. 4.109PCh. 4 - Predict the product(s) and write a balanced...Ch. 4 - Prob. 4.111PCh. 4 - Predict the product(s) and write a balanced...Ch. 4 - How many grams of O2 can be prepared from the...Ch. 4 - How many grams of chlorine gas can be produced...Ch. 4 - Prob. 4.115PCh. 4 - Prob. 4.116PCh. 4 - A mixture of KClO3 and KCl with a mass of 0.950 g...Ch. 4 - Prob. 4.118PCh. 4 - Before arc welding was developed, a displacement...Ch. 4 - Iron reacts rapidly with chlorine gas to form a...Ch. 4 - A sample of impure magnesium was analyzed by...Ch. 4 - Why is the equilibrium state said to be...Ch. 4 - Prob. 4.123PCh. 4 - Describe what happens on the molecular level when...Ch. 4 - When either a mixture of NO and Br2 or pure...Ch. 4 - Prob. 4.126PCh. 4 - Nutritional biochemists have known for decades...Ch. 4 - Limestone (CaCO3) is used to remove acidic...Ch. 4 - The brewing industry uses yeast to convert glucose...Ch. 4 - A chemical engineer determines the mass percent of...Ch. 4 - Prob. 4.131PCh. 4 - You are given solutions of HCl and NaOH and must...Ch. 4 - The flask represents the products of the titration...Ch. 4 - To find the mass percent of dolomite [CaMg(CO3)2]...Ch. 4 - On a lab exam, you have to find the concentrations...Ch. 4 - Nitric acid, a major industrial and laboratory...Ch. 4 - Prob. 4.137PCh. 4 - In 1995, Mario Molina, Paul Crutzen, and F....Ch. 4 - Sodium peroxide (Na2O2) is often used in...Ch. 4 - A student forgets to weigh a mixture of sodium...Ch. 4 - Prob. 4.141PCh. 4 - Prob. 4.142PCh. 4 - Physicians who specialize in sports medicine...Ch. 4 - Thyroxine (C15H11I4NO4) is a hormone synthesized...Ch. 4 - Over time, as their free fatty acid (FFA) content...Ch. 4 - Prob. 4.146PCh. 4 - Calcium dihydrogen phosphate, Ca(H2PO4)2, and...Ch. 4 - Prob. 4.148PCh. 4 - Prob. 4.149PCh. 4 - Prob. 4.150PCh. 4 - In 1997 and 2009, at United Nations conferences on...Ch. 4 - In a car engine, gasoline (represented by C8H18)...Ch. 4 - Prob. 4.153PCh. 4 - Prob. 4.154PCh. 4 - Prob. 4.155PCh. 4 - Prob. 4.156PCh. 4 - Prob. 4.157P
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