Chemistry: The Molecular Science
Chemistry: The Molecular Science
5th Edition
ISBN: 9781285199047
Author: John W. Moore, Conrad L. Stanitski
Publisher: Cengage Learning
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Chapter 17, Problem 17.ACP

(a)

Interpretation Introduction

Interpretation:

The combustion reaction for one mole of octane has to be stated.

Concept Introduction:

The chemical reactions in which an organic compound reacts with oxygen and produces carbon dioxide and water are referred to as combustion reactions.  These types of chemical reactions are exothermic in nature as large amount of heat is also produced as by product of the reaction.

(a)

Expert Solution
Check Mark

Answer to Problem 17.ACP

The chemical equation for complete combustion reaction of octane is shown below.

  C8H18+252O28CO2+9H2O

Explanation of Solution

The main products produced by the complete combustion of octane are carbon dioxide and water.  The chemical equation representing the combustion reaction of octane is shown below.

  C8H18+252O28CO2+9H2O

The chemical reaction shown above illustrates the burning of one mole of the octane in the presence of the oxygen to produce eight moles of carbon dioxide and nine moles of water.

(b)

Interpretation Introduction

Interpretation:

The chemical reaction for the hydrogenation process has to be stated.  Also the amount of hydrogen gas produced by the combustion of one mole of octane has to be determined.

Concept Introduction:

The chemical reaction which takes place between molecular hydrogen and another compound, in the presence of a catalyst such as nickel, palladium or platinum is termed as hydrogenation reaction.  This process is commonly used to reduce the unsaturated compounds.

(b)

Expert Solution
Check Mark

Answer to Problem 17.ACP

The chemical equation which represents the first step is shown below.

  C8H18+4O28CO+9H2

The chemical equation which represents the second step is shown below.

  8CO+8H2O8CO2+8H2

Seventeen moles of H2 are produced by the combustion of one mole of octane.

Explanation of Solution

The steps which include the hydrogenation process are shown below.

The first step is the partial oxidation of the octane which leads to the formation of carbon monoxide and hydrogen.

The chemical equation which represents the first step is shown below.

  C8H18+4O28CO+9H2

The second step leads to the production of carbon dioxide and hydrogen gas when carbon monoxide combines with water.  The mixture of gas obtained by the combination of carbon dioxide and hydrogen gas is referred to as the shift gas.

The chemical equation which represents the second step is shown below.

  8CO+8H2O8CO2+8H2

Hence the overall reaction will get on addition of chemical equation for first and second step which is shown below.

  C8H18+4O28CO+9H28CO+8H2O8CO2+8H2              _C8H18+4O2+8H2O8CO2+17H2

Thus, the overall reaction so obtained is shown below.

  C8H18+4O2+8H2O8CO2+17H2

According to the above chemical equation, seventeen moles of H2 are produced by the combustion of one mole of octane.

(c)

Interpretation Introduction

Interpretation:

The chemical equations are to be combined and have to be shown that the overall reaction is same as that of the combustion of octane.

Concept Introduction:

The zero-emission fuel burned with oxygen is referred to as hydrogen fuel.  There are many applications of it as it is used in fuel cells or internal combustion engines.  The hydrogen reacts with oxygen and leads to the formation of water and also releases energy as the by product.

(c)

Expert Solution
Check Mark

Answer to Problem 17.ACP

The result is same as that for the combustion reaction of octane.

Explanation of Solution

The chemical equation representing the reaction takes place for the hydrogen gas as a fuel is shown below.

  17H2+172O217H2O

The overall chemical equation so obtained in part (b) is shown below.

  C8H18+4O2+8H2O8CO2+17H2

The chemical equation for the combustion reaction of octane is obtained by addition of reactions mentioned above.  Thus, the result obtained is shown below.

  17H2+172O217H2OC8H18+4O2+8H2O8CO2+17H2_C8H18+252O28CO2+9H2O

Hence, the result so obtained by the addition of above two reactions is the same as the combustion reaction of octane.

(d)

Interpretation Introduction

Interpretation:

The Gibbs energy produced in thehydrogen fuel gas reaction and that of the combustion of the octane has to be compared.

Concept Introduction:

The general expression for the calculation of Gibbs free energy for a reaction is shown below.

  ΔGf={(Molesofproduct)×ΔGf(product)} {(Molesofreactant)×ΔGf(reactant)}

(d)

Expert Solution
Check Mark

Answer to Problem 17.ACP

The Gibbs energy produced in thehydrogen fuel gas reaction is less negative and has smaller magnitude as compared to the combustion of the octane.

Explanation of Solution

The chemical equation representing the combustion reaction of octane is shown below.

  C8H18+252O28CO2+9H2O

The elements which are present in their elemental states have ΔGf=0.  Thus, the standard Gibbs free energy for the formation of oxygen, ΔGf.O2(g) is 0.

The standard Gibbs free energy for the formation of water, ΔGf.H2O(g), octane, ΔGf.C8H18(g) and carbon dioxide, ΔGf.CO2(g) is 228.572kJ/mol, 6.707kJ/mol and 394.359kJ/mol respectively.

The expression for the calculation of Gibbs free energy for the combustion reaction of octane is shown below.

  ΔGf=(((8mol)ΔGf(CO2)+(9mol)ΔGf(H2O))((252mol)ΔGf(O2)+(1mol)ΔGf(C8H18)))        (1)

The value of ΔGf(CO2) is 394.359kJ/mol.

The value of ΔGf(H2O) is 228.572kJ/mol.

The value of ΔGf(O2) is 0.

The value of ΔGf(C8H18) is 6.707kJ/mol.

Substitute the value of ΔGf(CO2), ΔGf(H2O), ΔGf(O2) and ΔGf(C8H18) in equation (1).

  ΔGf=(((8mol)(394.359kJ/mol)+(9mol)(228.572kJ/mol))((252mol)(0)+(1mol)(6.707kJ/mol)))=3154.872kJ2057.148kJ6.707kJ=5218.727kJ

Thus, the energy produced during the combustion of one mole of octane is 5218.727kJ.

The chemical equation for the hydrogen gas shift reaction is shown below.

  17H2+172O217H2O

The elements which are present in their elemental states have ΔGf=0.  Thus, the standard Gibbs free energy for the formation of both oxygen, ΔGf.O2(g) and hydrogen, ΔGf.H2(g) is 0.

The standard Gibbs free energy for the formation of water, ΔGf.H2O(g) is 228.572kJ/mol.

The expression for the calculation of Gibbs free energy for the hydrogen gas shift reaction is shown below.

  ΔGf=((17mol)ΔGf(H2O)((172mol)ΔGf(O2)+(17mol)ΔGf(H2)))        (2)

The value of ΔGf(H2O) is 228.572kJ/mol.

The value of ΔGf(O2) is 0.

The value of ΔGf(H2) is 0.

Substitute the value of ΔGf(H2O), ΔGf(O2) and ΔGf(H2) in equation (2).

  ΔGf={(17mol)(228.572kJ/mol)}{(172mol)(0)+(17mol)(0)}=3885.724kJ

Thus, the energy produced during the hydrogen gas shift reaction is 3885.724kJ.

Therefore, the amount of the Gibbs energy produced in the hydrogen fuel gas reaction is less negative and has smaller magnitude as compared to that of the combustion of the octane.

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Chapter 17 Solutions

Chemistry: The Molecular Science

Ch. 17.4 - Given this reaction, its standard potential, and...Ch. 17.5 - Prob. 17.5PSPCh. 17.5 - Prob. 17.8CECh. 17.5 - Prob. 17.9CECh. 17.5 - Prob. 17.10CECh. 17.6 - Prob. 17.6PSPCh. 17.6 - Prob. 17.11ECh. 17.6 - Prob. 17.7PSPCh. 17.7 - Calculate the cell potential for the Zn(s) +...Ch. 17.7 - Prob. 17.9PSPCh. 17.8 - Prob. 17.12ECh. 17.8 - Prob. 17.13ECh. 17.8 - Prob. 17.14ECh. 17.10 - Predict the results of passing a direct electrical...Ch. 17.10 - In 1886. Henri Moissan was the first to prepare...Ch. 17.11 - In the commercial production of sodium metal by...Ch. 17.11 - Prob. 17.16CECh. 17.11 - Prob. 17.17ECh. 17.11 - Prob. 17.18CECh. 17.11 - Prob. 17.19ECh. 17.12 - Prob. 17.20CECh. 17.12 - Prob. 17.21CECh. 17 - Prob. 2SPCh. 17 - Prob. 1QRTCh. 17 - Prob. 2QRTCh. 17 - Prob. 3QRTCh. 17 - Prob. 4QRTCh. 17 - Identify each statement as true or false. Rewrite...Ch. 17 - Prob. 6QRTCh. 17 - Prob. 7QRTCh. 17 - Prob. 8QRTCh. 17 - Answer Question 8 again, but this time find a...Ch. 17 - Prob. 10QRTCh. 17 - Prob. 11QRTCh. 17 - For the reaction in Question 6, write balanced...Ch. 17 - Prob. 13QRTCh. 17 - Prob. 14QRTCh. 17 - Prob. 15QRTCh. 17 - Prob. 16QRTCh. 17 - Prob. 17QRTCh. 17 - For the reaction Cu2+(aq) + Zn(s) → Cu(s) + Zn2+...Ch. 17 - Prob. 19QRTCh. 17 - Prob. 20QRTCh. 17 - Prob. 21QRTCh. 17 - Prob. 22QRTCh. 17 - Draw a diagram of each cell. Label the anode, the...Ch. 17 - Prob. 24QRTCh. 17 - Prob. 25QRTCh. 17 - Prob. 26QRTCh. 17 - Prob. 27QRTCh. 17 - Prob. 28QRTCh. 17 - Prob. 29QRTCh. 17 - Prob. 30QRTCh. 17 - Prob. 31QRTCh. 17 - Consider these half-reactions: (a) Which is the...Ch. 17 - Consider these half-reactions: (a) Which is the...Ch. 17 - In principle, a battery could be made from...Ch. 17 - Prob. 35QRTCh. 17 - Hydrazine, N2H4, can be used as the reducing agent...Ch. 17 - Prob. 37QRTCh. 17 - Prob. 38QRTCh. 17 - Prob. 39QRTCh. 17 - Prob. 40QRTCh. 17 - Prob. 41QRTCh. 17 - Prob. 42QRTCh. 17 - Prob. 43QRTCh. 17 - Prob. 44QRTCh. 17 - Prob. 45QRTCh. 17 - Prob. 46QRTCh. 17 - Consider the voltaic cell 2 Ag+(aq) + Cd(s) 2...Ch. 17 - Consider a voltaic cell with the reaction H2(g) +...Ch. 17 - Calculate the cell potential of a concentration...Ch. 17 - Prob. 50QRTCh. 17 - Prob. 51QRTCh. 17 - Prob. 52QRTCh. 17 - Prob. 53QRTCh. 17 - NiCad batteries are rechargeable and are commonly...Ch. 17 - Prob. 55QRTCh. 17 - Prob. 56QRTCh. 17 - Prob. 57QRTCh. 17 - Hydrazine, N2H4, has been proposed as the fuel in...Ch. 17 - Consider the electrolysis of water in the presence...Ch. 17 - Prob. 60QRTCh. 17 - Prob. 61QRTCh. 17 - Prob. 62QRTCh. 17 - Identify the products of the electrolysis of a 1-M...Ch. 17 - Prob. 64QRTCh. 17 - Prob. 65QRTCh. 17 - Prob. 66QRTCh. 17 - Prob. 67QRTCh. 17 - Prob. 68QRTCh. 17 - Prob. 69QRTCh. 17 - Prob. 70QRTCh. 17 - Prob. 71QRTCh. 17 - Prob. 72QRTCh. 17 - Prob. 73QRTCh. 17 - Prob. 74QRTCh. 17 - Calculate how long it would take to electroplate a...Ch. 17 - Prob. 76QRTCh. 17 - Prob. 77QRTCh. 17 - Prob. 78QRTCh. 17 - Prob. 79QRTCh. 17 - Prob. 80QRTCh. 17 - Prob. 81QRTCh. 17 - Prob. 82QRTCh. 17 - Prob. 83QRTCh. 17 - Prob. 84QRTCh. 17 - Prob. 85QRTCh. 17 - Prob. 86QRTCh. 17 - Prob. 87QRTCh. 17 - Prob. 88QRTCh. 17 - You wish to electroplate a copper surface having...Ch. 17 - Prob. 90QRTCh. 17 - Prob. 91QRTCh. 17 - Prob. 92QRTCh. 17 - Prob. 93QRTCh. 17 - An electrolytic cell is set up with Cd(s) in...Ch. 17 - Prob. 95QRTCh. 17 - Prob. 96QRTCh. 17 - Prob. 97QRTCh. 17 - Prob. 98QRTCh. 17 - Prob. 99QRTCh. 17 - Prob. 100QRTCh. 17 - Prob. 101QRTCh. 17 - Prob. 102QRTCh. 17 - Prob. 103QRTCh. 17 - Prob. 104QRTCh. 17 - Prob. 105QRTCh. 17 - Prob. 106QRTCh. 17 - Prob. 107QRTCh. 17 - Prob. 108QRTCh. 17 - Prob. 109QRTCh. 17 - Prob. 110QRTCh. 17 - Prob. 111QRTCh. 17 - Prob. 17.ACPCh. 17 - Prob. 17.BCP
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