Chemistry: The Molecular Nature of Matter and Change
Chemistry: The Molecular Nature of Matter and Change
8th Edition
ISBN: 9781259631757
Author: Martin Silberberg Dr., Patricia Amateis Professor
Publisher: McGraw-Hill Education
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Chapter 4, Problem 4.126P

(a)

Interpretation Introduction

Interpretation:

The percent yield of the formation of NH3 is to be calculated.

Concept introduction:

Haber process is one of the industrial methods employed for the preparation of ammonia (NH3). In this method, nitrogen and hydrogen molecule react in the presence of an iron catalyst to form ammonia gas. High temperature and pressure condition is required for the reaction. The balanced chemical equation for the preparation of NH3 is:

N2(g)+3H2(g)2NH3(g)

Combination redox reactions are the reactions in which two or more reactants combine to form a single product. The formation of ammonia from nitrogen and hydrogen molecule is an example of a combination redox reaction.

(a)

Expert Solution
Check Mark

Answer to Problem 4.126P

The percent yield of the formation of NH3 is 61.7%.

Explanation of Solution

The mass of N2 is 20g.

The mass of H2 is 10g.

The mass of NH3 at equilibrium is 15g.

Nitrogen molecule (N2) reacts with hydrogen molecule (H2) to form ammonia molecule (NH3). The balanced chemical equation of the combination redox reaction is:

N2(g)+3H2(g)2NH3(g)

One mole of N2 reacts with three moles of H2 to give two moles of NH3.

The molecular mass of N2 is 28.02g/mol and the molecular mass of H2 is 2.016g/mol.

The formula to calculate moles of NH3 when N2 is limiting reagent is:

MolesofNH3=[(mass ofN2(g)molecular massofN2(g/mol))(2molNH31molN2)]                       (1)

Substitute 20g for the mass of N2 and 28.02g/mol for molecular mass of N2 in the equation (1).

MolesofNH3=[(20g28.02g/mol)(2molNH31molN2)]=[(0.713775mol)(2molNH31molN2)]=1.42755mol

The formula to calculate moles of NH3 when H2 is limiting reagent is:

MolesofNH3=[(mass ofH2(g)molecular massofH2(g/mol))(2molNH33molH2)]                        (2)

Substitute 10g for the mass of H2 and 2.016g/mol for molecular mass of H2 in the equation (2).

MolesofNH3=[(10g2.016g/mol)(2molNH33molH2)]=[(4.9603mol)(2molNH33molH2)]=3.306878mol

N2 is limiting reagent in the reaction as the moles of NH3 produced is less in this case as compared to when H2 is the limiting agent.

The molecular mass of NH3 is 17.03g/mol.

The formula to calculate the mass of NH3 is:

MassofNH3=(moles ofNH3(mol))(molecular mass of NH3(g/mol)) (3)

Substitute 1.42755mol for moles of NH3 and 17.03g/mol for molecular mass of NH3 in equation (3).

MassofFe=(1.42755mol)(17.03g/mol)=24.311g

The expression to calculate the percent yield of the reaction is:

 %yield=(actual yield(g)theoretical yield(g))(100) (4)

Substitute 15g for actual yield and 24.311g for theoretical yield in the equation (4).

 %yield=(15g24.311g)(100)=61.7%

Conclusion

The percent yield of the formation of NH3 is 61.7%.

(b)

Interpretation Introduction

Interpretation:

The moles of N2 and H2 that are present at equilibrium 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 decomposes to form one or more product.

(b)

Expert Solution
Check Mark

Answer to Problem 4.126P

The moles of N2 and H2 that are present at equilibrium is 0.273mol and 3.64mol respectively.

Explanation of Solution

The mass of N2 is 20g.

The mass of H2 is 10g.

The mass of NH3 at equilibrium is 15g.

The molecular mass of N2 is 28.02g/mol and the molecular mass of H2 is 2.0916g/mol.

The formula to calculate moles of N2 initially present in the reaction is:

MolesofN2=(mass ofN2(g)molecular massofN2(g/mol))                                                    (5)

Substitute 20g for the mass of N2 and 28.02g/mol for molecular mass of N2 in the equation (5).

MolesofN2=(20g28.02g/mol)=0.71378mol

The formula to calculate moles of H2 initially present in the reaction is:

MolesofH2=(mass ofH2(g)molecular massofH2(g/mol))                                                     (6)

Substitute 10g for the mass of H2 and 2.016g/mol for molecular mass of H2 in the equation (6).

MolesofH2=(10g2.016g/mol)=4.9603mol

The molecular mass of NH3 is 17.03g/mol.

The formula to calculate moles of N2 to produce 15gNH3 is:

MolesofN2=[(mass ofNH3(g)molecular massofNH3(g/mol))(1molN22molNH3)]                       (7)

Substitute 15g for the mass of NH3 and 17.03g/mol for molecular mass of NH3 in the equation (7).

MolesofN2=[(15g17.03g/mol)(1molN22molNH3)]=0.4404mol

The formula to calculate moles of H2 to produce 15gNH3 is:

MolesofH2=[(mass ofNH3(g)molecular massofNH3(g/mol))(3molH22molNH3)]                       (8)

Substitute 15g for the mass of NH3 and 17.03g/mol for molecular mass of NH3 in the equation (8).

MolesofH2=[(15g17.03g/mol)(3molH22molNH3)]=1.3212mol

The formula to calculate moles of N2 at equilibrium is:

Moles of N2 at equilibrium=(Initial moles ofN2)(Reacted mole ofN2) (9)

Substitute 0.71378mol for an initial mole of N2 and 0.4404mol for a reacted mole of N2 in the equation (9).

Moles of N2 at equilibrium=(0.71378mol)(0.4404mol)=0.27338mol0.273mol

The formula to calculate moles of H2 at equilibrium is:

Moles of H2 at equilibrium=(Initial moles ofH2)(Reacted mole ofH2) (10)

Substitute 4.9603mol for an initial mole of H2 and 1.3212mol for a reacted mole of H2 in the equation (10).

Moles of N2 at equilibrium=(4.9603mol)(1.3212mol)=3.6391mol3.64mol

Conclusion

The moles of N2 and H2 that are present at equilibrium is 0.273mol and 3.64mol respectively.

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Chapter 4 Solutions

Chemistry: The Molecular Nature of Matter and Change

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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