Methane, CH 4 , can be converted to methanol, which, like ethanol, can be used as a fuel. The energy level diagram shown here presents relationships between energies of the fuels and their oxidation products. Use the information in the diagram to answer the following questions. (The energy terms are per mol-rxn.) (a) Which fuel, methanol or methane, yields the most energy per mole when burned? (b) Which fuel yields the most energy per gram when burned? (c) What is the enthalpy change for the conversion of methane to methanol by reaction with O 2 (g)? (d) Each arrow on the diagram represents a chemical reaction . Write the equation for the reaction that converts methane to methanol.

Question

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Answer 1

Textbook Question

Chapter 5, Problem 115SCQ

Methane, CH₄, can be converted to methanol, which, like ethanol, can be used as a fuel. The energy level diagram shown here presents relationships between energies of the fuels and their oxidation products. Use the information in the diagram to answer the following questions. (The energy terms are per mol-rxn.)

Chapter 5, Problem 115SCQ, Methane, CH4, can be converted to methanol, which, like ethanol, can be used as a fuel. The energy

(a) Which fuel, methanol or methane, yields the most energy per mole when burned?
(b) Which fuel yields the most energy per gram when burned?
(c) What is the enthalpy change for the conversion of methane to methanol by reaction with O₂(g)?
(d) Each arrow on the diagram represents a chemical reaction. Write the equation for the reaction that converts methane to methanol.

(a)

Expert Solution

Interpretation Introduction

Interpretation:

The fuel that yields the most energy per mole when burned has to be determined

Concept Introduction:

Heat energy required to raise the temperature of 1g of substance by 1K.Energy gained or lost can be calculated using the below equation.

$q=C×m×ΔT$

Where, q= energy gained or lost for a given mass of substance (m), C =specific heat capacity, $ΔT$ = change in temperature.

The standard molar enthalpy of formation is the enthalpy change $ΔfH0$ is the enthalpy change for the formation of $1mol$ of a compound directly from its component elements in their standard states. And is given by

$ΔrH0$ Pac Mindlink Owlv2 (24 Months) Chemistry & Chemical Reactivity 9e, Chapter 5, Problem 115SCQ , additional homework tip 1 $ΣnΔfH0(products) - ΣnΔfH0(reactants)$

Explanation of Solution

From the energy level diagram,

Methane liberates at $955.1kJ/mol$

Methanol liberates at $676.1kJ/mol$

So, methane yields most energy per mole when it’s burned.

(b)

Expert Solution

Interpretation Introduction

Interpretation:

The fuel yields the most energy per gram when burned has to be calculated.

Concept Introduction:

Heat energy required to raise the temperature of 1g of substance by 1K.Energy gained or lost can be calculated using the below equation.

$q=C×m×ΔT$

Where, q= energy gained or lost for a given mass of substance (m), C =specific heat capacity, $ΔT$ = change in temperature.

The standard molar enthalpy of formation is the enthalpy change $ΔfH0$ is the enthalpy change for the formation of $1mol$ of a compound directly from its component elements in their standard states. And is given by

$ΔrH0$ Pac Mindlink Owlv2 (24 Months) Chemistry & Chemical Reactivity 9e, Chapter 5, Problem 115SCQ , additional homework tip 2 $ΣnΔfH0(products) - ΣnΔfH0(reactants)$

Explanation of Solution

The fuel yields the most energy per gram when burned

Molar mass of methane is $16.04 g/mol$

For methane= $-955.1kJ1mol×1mol16.04g$ = $-59.54kJ/g$

Molar mass of methanol is $32.04 g/mol$

For methanol= $-676.1kJ1mol×1mol32.04g$ = $-21.10kJ/g$

So, the fuel that yields the most energy per gram when burned is methane

(c)

Expert Solution

Interpretation Introduction

Interpretation:

The enthalpy change for the conversion of methane by reaction with $O2(g)$ has to be determined.

Concept Introduction:

Heat energy required to raise the temperature of 1g of substance by 1K. Energy gained or lost can be calculated using the below equation.

$q=C×m×ΔT$

Where, q= energy gained or lost for a given mass of substance (m), C =specific heat capacity, $ΔT$ = change in temperature.

The standard enthalpy change of combustion of a compound is the enthalpy change which occurs when one gram of the compound is burned completely in oxygen under standard conditions, and with everything in its standard state.

$ΔrH0$ = $ΣnΔfH0(products) - ΣnΔfH0(reactants)$

Explanation of Solution

From the energy level diagram the values obtained are

Methane liberates at $955.1kJ/mol$

Methanol liberates at $676.1kJ/mol$

$ΔrH0$ = $ΣnΔfH0(products) - ΣnΔfH0(reactants)$

$ΔrH$ = $-955.1kJ/mol -(-676.1kJ/mol)$ = $-278.9kJ/mol$

(d)

Expert Solution

Interpretation Introduction

Interpretation:

The equation for the reaction that converts methane to methanol has to be identified.

Concept Introduction:

Heat energy required to raise the temperature of 1g of substance by 1K. Energy gained or lost can be calculated using the below equation.

$q=C×m×ΔT$

Where, q= energy gained or lost for a given mass of substance (m), C =specific heat capacity, $ΔT$ = change in temperature.

The standard enthalpy change of combustion of a compound is the enthalpy change which occurs when one gram of the compound is burned completely in oxygen under standard conditions, and with everything in its standard state.

$ΔrH0$ = $ΣnΔfH0(products) - ΣnΔfH0(reactants)$

Explanation of Solution

From the energy level diagram the obtained equation for the conversion of methane to methanol is $CH4 + 2O2 → CH3OH$

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Answer 2

Textbook Question

Chapter 5, Problem 115SCQ

Methane, CH₄, can be converted to methanol, which, like ethanol, can be used as a fuel. The energy level diagram shown here presents relationships between energies of the fuels and their oxidation products. Use the information in the diagram to answer the following questions. (The energy terms are per mol-rxn.)

Chapter 5, Problem 115SCQ, Methane, CH4, can be converted to methanol, which, like ethanol, can be used as a fuel. The energy

(a) Which fuel, methanol or methane, yields the most energy per mole when burned?
(b) Which fuel yields the most energy per gram when burned?
(c) What is the enthalpy change for the conversion of methane to methanol by reaction with O₂(g)?
(d) Each arrow on the diagram represents a chemical reaction. Write the equation for the reaction that converts methane to methanol.

(a)

Expert Solution

Interpretation Introduction

Interpretation:

The fuel that yields the most energy per mole when burned has to be determined

Concept Introduction:

Heat energy required to raise the temperature of 1g of substance by 1K.Energy gained or lost can be calculated using the below equation.

$q=C×m×ΔT$

Where, q= energy gained or lost for a given mass of substance (m), C =specific heat capacity, $ΔT$ = change in temperature.

The standard molar enthalpy of formation is the enthalpy change $ΔfH0$ is the enthalpy change for the formation of $1mol$ of a compound directly from its component elements in their standard states. And is given by

$ΔrH0$ Pac Mindlink Owlv2 (24 Months) Chemistry & Chemical Reactivity 9e, Chapter 5, Problem 115SCQ , additional homework tip 1 $ΣnΔfH0(products) - ΣnΔfH0(reactants)$

Explanation of Solution

From the energy level diagram,

Methane liberates at $955.1kJ/mol$

Methanol liberates at $676.1kJ/mol$

So, methane yields most energy per mole when it’s burned.

(b)

Expert Solution

Interpretation Introduction

Interpretation:

The fuel yields the most energy per gram when burned has to be calculated.

Concept Introduction:

Heat energy required to raise the temperature of 1g of substance by 1K.Energy gained or lost can be calculated using the below equation.

$q=C×m×ΔT$

Where, q= energy gained or lost for a given mass of substance (m), C =specific heat capacity, $ΔT$ = change in temperature.

The standard molar enthalpy of formation is the enthalpy change $ΔfH0$ is the enthalpy change for the formation of $1mol$ of a compound directly from its component elements in their standard states. And is given by

$ΔrH0$ Pac Mindlink Owlv2 (24 Months) Chemistry & Chemical Reactivity 9e, Chapter 5, Problem 115SCQ , additional homework tip 2 $ΣnΔfH0(products) - ΣnΔfH0(reactants)$

Explanation of Solution

The fuel yields the most energy per gram when burned

Molar mass of methane is $16.04 g/mol$

For methane= $-955.1kJ1mol×1mol16.04g$ = $-59.54kJ/g$

Molar mass of methanol is $32.04 g/mol$

For methanol= $-676.1kJ1mol×1mol32.04g$ = $-21.10kJ/g$

So, the fuel that yields the most energy per gram when burned is methane

(c)

Expert Solution

Interpretation Introduction

Interpretation:

The enthalpy change for the conversion of methane by reaction with $O2(g)$ has to be determined.

Concept Introduction:

Heat energy required to raise the temperature of 1g of substance by 1K. Energy gained or lost can be calculated using the below equation.

$q=C×m×ΔT$

Where, q= energy gained or lost for a given mass of substance (m), C =specific heat capacity, $ΔT$ = change in temperature.

The standard enthalpy change of combustion of a compound is the enthalpy change which occurs when one gram of the compound is burned completely in oxygen under standard conditions, and with everything in its standard state.

$ΔrH0$ = $ΣnΔfH0(products) - ΣnΔfH0(reactants)$

Explanation of Solution

From the energy level diagram the values obtained are

Methane liberates at $955.1kJ/mol$

Methanol liberates at $676.1kJ/mol$

$ΔrH0$ = $ΣnΔfH0(products) - ΣnΔfH0(reactants)$

$ΔrH$ = $-955.1kJ/mol -(-676.1kJ/mol)$ = $-278.9kJ/mol$

(d)

Expert Solution

Interpretation Introduction

Interpretation:

The equation for the reaction that converts methane to methanol has to be identified.

Concept Introduction:

Heat energy required to raise the temperature of 1g of substance by 1K. Energy gained or lost can be calculated using the below equation.

$q=C×m×ΔT$

Where, q= energy gained or lost for a given mass of substance (m), C =specific heat capacity, $ΔT$ = change in temperature.

The standard enthalpy change of combustion of a compound is the enthalpy change which occurs when one gram of the compound is burned completely in oxygen under standard conditions, and with everything in its standard state.

$ΔrH0$ = $ΣnΔfH0(products) - ΣnΔfH0(reactants)$

Explanation of Solution

From the energy level diagram the obtained equation for the conversion of methane to methanol is $CH4 + 2O2 → CH3OH$

Want to see more full solutions like this?

Subscribe now to access step-by-step solutions to millions of textbook problems written by subject matter experts!

Answer 3

Textbook Question

Chapter 5, Problem 115SCQ

Methane, CH₄, can be converted to methanol, which, like ethanol, can be used as a fuel. The energy level diagram shown here presents relationships between energies of the fuels and their oxidation products. Use the information in the diagram to answer the following questions. (The energy terms are per mol-rxn.)

Chapter 5, Problem 115SCQ, Methane, CH4, can be converted to methanol, which, like ethanol, can be used as a fuel. The energy

(a) Which fuel, methanol or methane, yields the most energy per mole when burned?
(b) Which fuel yields the most energy per gram when burned?
(c) What is the enthalpy change for the conversion of methane to methanol by reaction with O₂(g)?
(d) Each arrow on the diagram represents a chemical reaction. Write the equation for the reaction that converts methane to methanol.

(a)

Expert Solution

Interpretation Introduction

Interpretation:

The fuel that yields the most energy per mole when burned has to be determined

Concept Introduction:

Heat energy required to raise the temperature of 1g of substance by 1K.Energy gained or lost can be calculated using the below equation.

$q=C×m×ΔT$

Where, q= energy gained or lost for a given mass of substance (m), C =specific heat capacity, $ΔT$ = change in temperature.

The standard molar enthalpy of formation is the enthalpy change $ΔfH0$ is the enthalpy change for the formation of $1mol$ of a compound directly from its component elements in their standard states. And is given by

$ΔrH0$ Pac Mindlink Owlv2 (24 Months) Chemistry & Chemical Reactivity 9e, Chapter 5, Problem 115SCQ , additional homework tip 1 $ΣnΔfH0(products) - ΣnΔfH0(reactants)$

Explanation of Solution

From the energy level diagram,

Methane liberates at $955.1kJ/mol$

Methanol liberates at $676.1kJ/mol$

So, methane yields most energy per mole when it’s burned.

(b)

Expert Solution

Interpretation Introduction

Interpretation:

The fuel yields the most energy per gram when burned has to be calculated.

Concept Introduction:

Heat energy required to raise the temperature of 1g of substance by 1K.Energy gained or lost can be calculated using the below equation.

$q=C×m×ΔT$

Where, q= energy gained or lost for a given mass of substance (m), C =specific heat capacity, $ΔT$ = change in temperature.

The standard molar enthalpy of formation is the enthalpy change $ΔfH0$ is the enthalpy change for the formation of $1mol$ of a compound directly from its component elements in their standard states. And is given by

$ΔrH0$ Pac Mindlink Owlv2 (24 Months) Chemistry & Chemical Reactivity 9e, Chapter 5, Problem 115SCQ , additional homework tip 2 $ΣnΔfH0(products) - ΣnΔfH0(reactants)$

Explanation of Solution

The fuel yields the most energy per gram when burned

Molar mass of methane is $16.04 g/mol$

For methane= $-955.1kJ1mol×1mol16.04g$ = $-59.54kJ/g$

Molar mass of methanol is $32.04 g/mol$

For methanol= $-676.1kJ1mol×1mol32.04g$ = $-21.10kJ/g$

So, the fuel that yields the most energy per gram when burned is methane

(c)

Expert Solution

Interpretation Introduction

Interpretation:

The enthalpy change for the conversion of methane by reaction with $O2(g)$ has to be determined.

Concept Introduction:

Heat energy required to raise the temperature of 1g of substance by 1K. Energy gained or lost can be calculated using the below equation.

$q=C×m×ΔT$

Where, q= energy gained or lost for a given mass of substance (m), C =specific heat capacity, $ΔT$ = change in temperature.

The standard enthalpy change of combustion of a compound is the enthalpy change which occurs when one gram of the compound is burned completely in oxygen under standard conditions, and with everything in its standard state.

$ΔrH0$ = $ΣnΔfH0(products) - ΣnΔfH0(reactants)$

Explanation of Solution

From the energy level diagram the values obtained are

Methane liberates at $955.1kJ/mol$

Methanol liberates at $676.1kJ/mol$

$ΔrH0$ = $ΣnΔfH0(products) - ΣnΔfH0(reactants)$

$ΔrH$ = $-955.1kJ/mol -(-676.1kJ/mol)$ = $-278.9kJ/mol$

(d)

Expert Solution

Interpretation Introduction

Interpretation:

The equation for the reaction that converts methane to methanol has to be identified.

Concept Introduction:

Heat energy required to raise the temperature of 1g of substance by 1K. Energy gained or lost can be calculated using the below equation.

$q=C×m×ΔT$

Where, q= energy gained or lost for a given mass of substance (m), C =specific heat capacity, $ΔT$ = change in temperature.

The standard enthalpy change of combustion of a compound is the enthalpy change which occurs when one gram of the compound is burned completely in oxygen under standard conditions, and with everything in its standard state.

$ΔrH0$ = $ΣnΔfH0(products) - ΣnΔfH0(reactants)$

Explanation of Solution

From the energy level diagram the obtained equation for the conversion of methane to methanol is $CH4 + 2O2 → CH3OH$

Want to see more full solutions like this?

Subscribe now to access step-by-step solutions to millions of textbook problems written by subject matter experts!

Answer 4

Textbook Question

Chapter 5, Problem 115SCQ

Methane, CH₄, can be converted to methanol, which, like ethanol, can be used as a fuel. The energy level diagram shown here presents relationships between energies of the fuels and their oxidation products. Use the information in the diagram to answer the following questions. (The energy terms are per mol-rxn.)

Chapter 5, Problem 115SCQ, Methane, CH4, can be converted to methanol, which, like ethanol, can be used as a fuel. The energy

(a) Which fuel, methanol or methane, yields the most energy per mole when burned?
(b) Which fuel yields the most energy per gram when burned?
(c) What is the enthalpy change for the conversion of methane to methanol by reaction with O₂(g)?
(d) Each arrow on the diagram represents a chemical reaction. Write the equation for the reaction that converts methane to methanol.

(a)

Expert Solution

Interpretation Introduction

Interpretation:

The fuel that yields the most energy per mole when burned has to be determined

Concept Introduction:

Heat energy required to raise the temperature of 1g of substance by 1K.Energy gained or lost can be calculated using the below equation.

$q=C×m×ΔT$

Where, q= energy gained or lost for a given mass of substance (m), C =specific heat capacity, $ΔT$ = change in temperature.

The standard molar enthalpy of formation is the enthalpy change $ΔfH0$ is the enthalpy change for the formation of $1mol$ of a compound directly from its component elements in their standard states. And is given by

$ΔrH0$ Pac Mindlink Owlv2 (24 Months) Chemistry & Chemical Reactivity 9e, Chapter 5, Problem 115SCQ , additional homework tip 1 $ΣnΔfH0(products) - ΣnΔfH0(reactants)$

Explanation of Solution

From the energy level diagram,

Methane liberates at $955.1kJ/mol$

Methanol liberates at $676.1kJ/mol$

So, methane yields most energy per mole when it’s burned.

(b)

Expert Solution

Interpretation Introduction

Interpretation:

The fuel yields the most energy per gram when burned has to be calculated.

Concept Introduction:

Heat energy required to raise the temperature of 1g of substance by 1K.Energy gained or lost can be calculated using the below equation.

$q=C×m×ΔT$

Where, q= energy gained or lost for a given mass of substance (m), C =specific heat capacity, $ΔT$ = change in temperature.

The standard molar enthalpy of formation is the enthalpy change $ΔfH0$ is the enthalpy change for the formation of $1mol$ of a compound directly from its component elements in their standard states. And is given by

$ΔrH0$ Pac Mindlink Owlv2 (24 Months) Chemistry & Chemical Reactivity 9e, Chapter 5, Problem 115SCQ , additional homework tip 2 $ΣnΔfH0(products) - ΣnΔfH0(reactants)$

Explanation of Solution

The fuel yields the most energy per gram when burned

Molar mass of methane is $16.04 g/mol$

For methane= $-955.1kJ1mol×1mol16.04g$ = $-59.54kJ/g$

Molar mass of methanol is $32.04 g/mol$

For methanol= $-676.1kJ1mol×1mol32.04g$ = $-21.10kJ/g$

So, the fuel that yields the most energy per gram when burned is methane

(c)

Expert Solution

Interpretation Introduction

Interpretation:

The enthalpy change for the conversion of methane by reaction with $O2(g)$ has to be determined.

Concept Introduction:

Heat energy required to raise the temperature of 1g of substance by 1K. Energy gained or lost can be calculated using the below equation.

$q=C×m×ΔT$

Where, q= energy gained or lost for a given mass of substance (m), C =specific heat capacity, $ΔT$ = change in temperature.

The standard enthalpy change of combustion of a compound is the enthalpy change which occurs when one gram of the compound is burned completely in oxygen under standard conditions, and with everything in its standard state.

$ΔrH0$ = $ΣnΔfH0(products) - ΣnΔfH0(reactants)$

Explanation of Solution

From the energy level diagram the values obtained are

Methane liberates at $955.1kJ/mol$

Methanol liberates at $676.1kJ/mol$

$ΔrH0$ = $ΣnΔfH0(products) - ΣnΔfH0(reactants)$

$ΔrH$ = $-955.1kJ/mol -(-676.1kJ/mol)$ = $-278.9kJ/mol$

(d)

Expert Solution

Interpretation Introduction

Interpretation:

The equation for the reaction that converts methane to methanol has to be identified.

Concept Introduction:

Heat energy required to raise the temperature of 1g of substance by 1K. Energy gained or lost can be calculated using the below equation.

$q=C×m×ΔT$

Where, q= energy gained or lost for a given mass of substance (m), C =specific heat capacity, $ΔT$ = change in temperature.

The standard enthalpy change of combustion of a compound is the enthalpy change which occurs when one gram of the compound is burned completely in oxygen under standard conditions, and with everything in its standard state.

$ΔrH0$ = $ΣnΔfH0(products) - ΣnΔfH0(reactants)$

Explanation of Solution

From the energy level diagram the obtained equation for the conversion of methane to methanol is $CH4 + 2O2 → CH3OH$

Want to see more full solutions like this?

Subscribe now to access step-by-step solutions to millions of textbook problems written by subject matter experts!

Answer 5

Textbook Question

Answer 6

Textbook Question

Answer 7

(a)

Expert Solution

Interpretation Introduction

Interpretation:

The fuel that yields the most energy per mole when burned has to be determined

Concept Introduction:

Heat energy required to raise the temperature of 1g of substance by 1K.Energy gained or lost can be calculated using the below equation.

$q=C×m×ΔT$

Where, q= energy gained or lost for a given mass of substance (m), C =specific heat capacity, $ΔT$ = change in temperature.

The standard molar enthalpy of formation is the enthalpy change $ΔfH0$ is the enthalpy change for the formation of $1mol$ of a compound directly from its component elements in their standard states. And is given by

$ΔrH0$ Pac Mindlink Owlv2 (24 Months) Chemistry & Chemical Reactivity 9e, Chapter 5, Problem 115SCQ , additional homework tip 1 $ΣnΔfH0(products) - ΣnΔfH0(reactants)$

Explanation of Solution

From the energy level diagram,

Methane liberates at $955.1kJ/mol$

Methanol liberates at $676.1kJ/mol$

So, methane yields most energy per mole when it’s burned.

(b)

Expert Solution

Interpretation Introduction

Interpretation:

The fuel yields the most energy per gram when burned has to be calculated.

Concept Introduction:

Heat energy required to raise the temperature of 1g of substance by 1K.Energy gained or lost can be calculated using the below equation.

$q=C×m×ΔT$

Where, q= energy gained or lost for a given mass of substance (m), C =specific heat capacity, $ΔT$ = change in temperature.

The standard molar enthalpy of formation is the enthalpy change $ΔfH0$ is the enthalpy change for the formation of $1mol$ of a compound directly from its component elements in their standard states. And is given by

$ΔrH0$ Pac Mindlink Owlv2 (24 Months) Chemistry & Chemical Reactivity 9e, Chapter 5, Problem 115SCQ , additional homework tip 2 $ΣnΔfH0(products) - ΣnΔfH0(reactants)$

Explanation of Solution

The fuel yields the most energy per gram when burned

Molar mass of methane is $16.04 g/mol$

For methane= $-955.1kJ1mol×1mol16.04g$ = $-59.54kJ/g$

Molar mass of methanol is $32.04 g/mol$

For methanol= $-676.1kJ1mol×1mol32.04g$ = $-21.10kJ/g$

So, the fuel that yields the most energy per gram when burned is methane

(c)

Expert Solution

Interpretation Introduction

Interpretation:

The enthalpy change for the conversion of methane by reaction with $O2(g)$ has to be determined.

Concept Introduction:

Heat energy required to raise the temperature of 1g of substance by 1K. Energy gained or lost can be calculated using the below equation.

$q=C×m×ΔT$

Where, q= energy gained or lost for a given mass of substance (m), C =specific heat capacity, $ΔT$ = change in temperature.

The standard enthalpy change of combustion of a compound is the enthalpy change which occurs when one gram of the compound is burned completely in oxygen under standard conditions, and with everything in its standard state.

$ΔrH0$ = $ΣnΔfH0(products) - ΣnΔfH0(reactants)$

Explanation of Solution

From the energy level diagram the values obtained are

Methane liberates at $955.1kJ/mol$

Methanol liberates at $676.1kJ/mol$

$ΔrH0$ = $ΣnΔfH0(products) - ΣnΔfH0(reactants)$

$ΔrH$ = $-955.1kJ/mol -(-676.1kJ/mol)$ = $-278.9kJ/mol$

(d)

Expert Solution

Interpretation Introduction

Interpretation:

The equation for the reaction that converts methane to methanol has to be identified.

Concept Introduction:

Heat energy required to raise the temperature of 1g of substance by 1K. Energy gained or lost can be calculated using the below equation.

$q=C×m×ΔT$

Where, q= energy gained or lost for a given mass of substance (m), C =specific heat capacity, $ΔT$ = change in temperature.

The standard enthalpy change of combustion of a compound is the enthalpy change which occurs when one gram of the compound is burned completely in oxygen under standard conditions, and with everything in its standard state.

$ΔrH0$ = $ΣnΔfH0(products) - ΣnΔfH0(reactants)$

Explanation of Solution

From the energy level diagram the obtained equation for the conversion of methane to methanol is $CH4 + 2O2 → CH3OH$

Answer 8

(a)

Expert Solution

Interpretation Introduction

Interpretation:

The fuel that yields the most energy per mole when burned has to be determined

Concept Introduction:

Heat energy required to raise the temperature of 1g of substance by 1K.Energy gained or lost can be calculated using the below equation.

$q=C×m×ΔT$

Where, q= energy gained or lost for a given mass of substance (m), C =specific heat capacity, $ΔT$ = change in temperature.

The standard molar enthalpy of formation is the enthalpy change $ΔfH0$ is the enthalpy change for the formation of $1mol$ of a compound directly from its component elements in their standard states. And is given by

$ΔrH0$ Pac Mindlink Owlv2 (24 Months) Chemistry & Chemical Reactivity 9e, Chapter 5, Problem 115SCQ , additional homework tip 1 $ΣnΔfH0(products) - ΣnΔfH0(reactants)$

Explanation of Solution

From the energy level diagram,

Methane liberates at $955.1kJ/mol$

Methanol liberates at $676.1kJ/mol$

So, methane yields most energy per mole when it’s burned.

Answer 9

(a)

Expert Solution

Answer 10

(a)

Expert Solution

Answer 11

Expert Solution

Answer 12

Interpretation Introduction

Interpretation:

The fuel that yields the most energy per mole when burned has to be determined

Concept Introduction:

Heat energy required to raise the temperature of 1g of substance by 1K.Energy gained or lost can be calculated using the below equation.

$q=C×m×ΔT$

Where, q= energy gained or lost for a given mass of substance (m), C =specific heat capacity, $ΔT$ = change in temperature.

The standard molar enthalpy of formation is the enthalpy change $ΔfH0$ is the enthalpy change for the formation of $1mol$ of a compound directly from its component elements in their standard states. And is given by

$ΔrH0$ Pac Mindlink Owlv2 (24 Months) Chemistry & Chemical Reactivity 9e, Chapter 5, Problem 115SCQ , additional homework tip 1 $ΣnΔfH0(products) - ΣnΔfH0(reactants)$

Answer 13

Explanation of Solution

From the energy level diagram,

Methane liberates at $955.1kJ/mol$

Methanol liberates at $676.1kJ/mol$

So, methane yields most energy per mole when it’s burned.

Answer 14

(b)

Expert Solution

Interpretation Introduction

Interpretation:

The fuel yields the most energy per gram when burned has to be calculated.

Concept Introduction:

Heat energy required to raise the temperature of 1g of substance by 1K.Energy gained or lost can be calculated using the below equation.

$q=C×m×ΔT$

Where, q= energy gained or lost for a given mass of substance (m), C =specific heat capacity, $ΔT$ = change in temperature.

The standard molar enthalpy of formation is the enthalpy change $ΔfH0$ is the enthalpy change for the formation of $1mol$ of a compound directly from its component elements in their standard states. And is given by

$ΔrH0$ Pac Mindlink Owlv2 (24 Months) Chemistry & Chemical Reactivity 9e, Chapter 5, Problem 115SCQ , additional homework tip 2 $ΣnΔfH0(products) - ΣnΔfH0(reactants)$

Explanation of Solution

The fuel yields the most energy per gram when burned

Molar mass of methane is $16.04 g/mol$

For methane= $-955.1kJ1mol×1mol16.04g$ = $-59.54kJ/g$

Molar mass of methanol is $32.04 g/mol$

For methanol= $-676.1kJ1mol×1mol32.04g$ = $-21.10kJ/g$

So, the fuel that yields the most energy per gram when burned is methane

Answer 15

(b)

Expert Solution

Answer 16

(b)

Expert Solution

Answer 17

Expert Solution

Answer 18

Interpretation Introduction

Interpretation:

The fuel yields the most energy per gram when burned has to be calculated.

Concept Introduction:

Heat energy required to raise the temperature of 1g of substance by 1K.Energy gained or lost can be calculated using the below equation.

$q=C×m×ΔT$

Where, q= energy gained or lost for a given mass of substance (m), C =specific heat capacity, $ΔT$ = change in temperature.

The standard molar enthalpy of formation is the enthalpy change $ΔfH0$ is the enthalpy change for the formation of $1mol$ of a compound directly from its component elements in their standard states. And is given by

$ΔrH0$ Pac Mindlink Owlv2 (24 Months) Chemistry & Chemical Reactivity 9e, Chapter 5, Problem 115SCQ , additional homework tip 2 $ΣnΔfH0(products) - ΣnΔfH0(reactants)$

Answer 19

Explanation of Solution

The fuel yields the most energy per gram when burned

Molar mass of methane is $16.04 g/mol$

For methane= $-955.1kJ1mol×1mol16.04g$ = $-59.54kJ/g$

Molar mass of methanol is $32.04 g/mol$

For methanol= $-676.1kJ1mol×1mol32.04g$ = $-21.10kJ/g$

So, the fuel that yields the most energy per gram when burned is methane

Answer 20

(c)

Expert Solution

Interpretation Introduction

Interpretation:

The enthalpy change for the conversion of methane by reaction with $O2(g)$ has to be determined.

Concept Introduction:

Heat energy required to raise the temperature of 1g of substance by 1K. Energy gained or lost can be calculated using the below equation.

$q=C×m×ΔT$

Where, q= energy gained or lost for a given mass of substance (m), C =specific heat capacity, $ΔT$ = change in temperature.

The standard enthalpy change of combustion of a compound is the enthalpy change which occurs when one gram of the compound is burned completely in oxygen under standard conditions, and with everything in its standard state.

$ΔrH0$ = $ΣnΔfH0(products) - ΣnΔfH0(reactants)$

Explanation of Solution

From the energy level diagram the values obtained are

Methane liberates at $955.1kJ/mol$

Methanol liberates at $676.1kJ/mol$

$ΔrH0$ = $ΣnΔfH0(products) - ΣnΔfH0(reactants)$

$ΔrH$ = $-955.1kJ/mol -(-676.1kJ/mol)$ = $-278.9kJ/mol$

Answer 21

(c)

Expert Solution

Answer 22

(c)

Expert Solution

Answer 23

Expert Solution

Answer 24

Interpretation Introduction

Interpretation:

The enthalpy change for the conversion of methane by reaction with $O2(g)$ has to be determined.

Concept Introduction:

Heat energy required to raise the temperature of 1g of substance by 1K. Energy gained or lost can be calculated using the below equation.

$q=C×m×ΔT$

Where, q= energy gained or lost for a given mass of substance (m), C =specific heat capacity, $ΔT$ = change in temperature.

The standard enthalpy change of combustion of a compound is the enthalpy change which occurs when one gram of the compound is burned completely in oxygen under standard conditions, and with everything in its standard state.

$ΔrH0$ = $ΣnΔfH0(products) - ΣnΔfH0(reactants)$

Answer 25

Explanation of Solution

From the energy level diagram the values obtained are

Methane liberates at $955.1kJ/mol$

Methanol liberates at $676.1kJ/mol$

$ΔrH0$ = $ΣnΔfH0(products) - ΣnΔfH0(reactants)$

$ΔrH$ = $-955.1kJ/mol -(-676.1kJ/mol)$ = $-278.9kJ/mol$

Answer 26

(d)

Expert Solution

Interpretation Introduction

Interpretation:

The equation for the reaction that converts methane to methanol has to be identified.

Concept Introduction:

Heat energy required to raise the temperature of 1g of substance by 1K. Energy gained or lost can be calculated using the below equation.

$q=C×m×ΔT$

Where, q= energy gained or lost for a given mass of substance (m), C =specific heat capacity, $ΔT$ = change in temperature.

The standard enthalpy change of combustion of a compound is the enthalpy change which occurs when one gram of the compound is burned completely in oxygen under standard conditions, and with everything in its standard state.

$ΔrH0$ = $ΣnΔfH0(products) - ΣnΔfH0(reactants)$

Explanation of Solution

From the energy level diagram the obtained equation for the conversion of methane to methanol is $CH4 + 2O2 → CH3OH$

Answer 27

(d)

Expert Solution

Answer 28

(d)

Expert Solution

Answer 29

Expert Solution

Answer 30

Interpretation Introduction

Interpretation:

The equation for the reaction that converts methane to methanol has to be identified.

Concept Introduction:

Heat energy required to raise the temperature of 1g of substance by 1K. Energy gained or lost can be calculated using the below equation.

$q=C×m×ΔT$

Where, q= energy gained or lost for a given mass of substance (m), C =specific heat capacity, $ΔT$ = change in temperature.

The standard enthalpy change of combustion of a compound is the enthalpy change which occurs when one gram of the compound is burned completely in oxygen under standard conditions, and with everything in its standard state.

$ΔrH0$ = $ΣnΔfH0(products) - ΣnΔfH0(reactants)$