Temperature condition is needed to be explained in the given dehydrogenation reaction. Concept introduction: Dehydrogenation: dehydrogenation is a process of elimination of hydrogen molecule from the substrate at high temperature condition. Free energy: reaction is feasible when free energy is negative. ΔG = ΔH-TΔS ΔG = free energy ΔH = change in enthalpy ΔS = change in entropy

Question

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Answer 1

Question

Chapter 9, Problem 48PP

Interpretation Introduction

Interpretation:

Temperature condition is needed to be explained in the given dehydrogenation reaction.

Concept introduction:

Dehydrogenation: dehydrogenation is a process of elimination of hydrogen molecule from the substrate at high temperature condition.

Free energy: reaction is feasible when free energy is negative.

ΔG = ΔH-TΔSΔG = free energyΔH = change in enthalpyΔS = change in entropy

Expert Solution & Answer

Answer to Problem 48PP

Reaction is feasible at higher temperature conditions only since ΔG is negative at higher temperatures. Therefore, higher temperatures are needed for dehydrogenation process.

Explanation of Solution

To explain: the conditions for the given reaction.

Given reaction is shown below.

ORGANIC CHEMISTRY GGC>CUSTOM<-TEXT, Chapter 9, Problem 48PP

Clear from the reaction that the ethane molecule converted ethylene molecule at high temperature condition by releasing hydrogen gas.

Given reaction refers the dehydrogenation process at high temperatures. Given substrate is ethane and this ethane molecule heated at high temperature (750⁰ C) to produce ethylene and hydrogen gas.

To give: the reason for high temperatures needed for the dehydrogenation process.

Given reaction is favorable when ΔG is negative and change in enthalpy is positive for this reaction because two sigma bonds are braking to form one pi-bond. In addition, change in entropy is positive because one molecule is converting into two molecules. So depending on these conditions, reaction temperature should be high then only ΔG will be negative to feasible this reaction.

ΔG = ΔH-TΔSΔH = -ve ΔS = +ve

At higher temperature condition, the given reaction is feasible since ΔG is negative.

Conclusion

Conclusion

At higher temperature conditions, value of free energy will be negative so the dehydrogenation reaction is feasible at higher temperature conditions.

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In the decomposition reaction in solution B → C, only species C absorbs UV radiation, but neither B nor the solvent absorbs. If we call At the absorbance measured at any time, A0 the absorbance at the beginning of the reaction, and A∞ the absorbance at the end of the reaction, which of the expressions is valid? We assume that Beer's law is fulfilled.

Answer 2

Question

Chapter 9, Problem 48PP

Interpretation Introduction

Interpretation:

Temperature condition is needed to be explained in the given dehydrogenation reaction.

Concept introduction:

Dehydrogenation: dehydrogenation is a process of elimination of hydrogen molecule from the substrate at high temperature condition.

Free energy: reaction is feasible when free energy is negative.

ΔG = ΔH-TΔSΔG = free energyΔH = change in enthalpyΔS = change in entropy

Expert Solution & Answer

Answer to Problem 48PP

Reaction is feasible at higher temperature conditions only since ΔG is negative at higher temperatures. Therefore, higher temperatures are needed for dehydrogenation process.

Explanation of Solution

To explain: the conditions for the given reaction.

Given reaction is shown below.

ORGANIC CHEMISTRY GGC>CUSTOM<-TEXT, Chapter 9, Problem 48PP

Clear from the reaction that the ethane molecule converted ethylene molecule at high temperature condition by releasing hydrogen gas.

Given reaction refers the dehydrogenation process at high temperatures. Given substrate is ethane and this ethane molecule heated at high temperature (750⁰ C) to produce ethylene and hydrogen gas.

To give: the reason for high temperatures needed for the dehydrogenation process.

Given reaction is favorable when ΔG is negative and change in enthalpy is positive for this reaction because two sigma bonds are braking to form one pi-bond. In addition, change in entropy is positive because one molecule is converting into two molecules. So depending on these conditions, reaction temperature should be high then only ΔG will be negative to feasible this reaction.

ΔG = ΔH-TΔSΔH = -ve ΔS = +ve

At higher temperature condition, the given reaction is feasible since ΔG is negative.

Conclusion

Conclusion

At higher temperature conditions, value of free energy will be negative so the dehydrogenation reaction is feasible at higher temperature conditions.

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

Question

Chapter 9, Problem 48PP

Interpretation Introduction

Interpretation:

Temperature condition is needed to be explained in the given dehydrogenation reaction.

Concept introduction:

Dehydrogenation: dehydrogenation is a process of elimination of hydrogen molecule from the substrate at high temperature condition.

Free energy: reaction is feasible when free energy is negative.

ΔG = ΔH-TΔSΔG = free energyΔH = change in enthalpyΔS = change in entropy

Expert Solution & Answer

Answer to Problem 48PP

Reaction is feasible at higher temperature conditions only since ΔG is negative at higher temperatures. Therefore, higher temperatures are needed for dehydrogenation process.

Explanation of Solution

To explain: the conditions for the given reaction.

Given reaction is shown below.

ORGANIC CHEMISTRY GGC>CUSTOM<-TEXT, Chapter 9, Problem 48PP

Clear from the reaction that the ethane molecule converted ethylene molecule at high temperature condition by releasing hydrogen gas.

Given reaction refers the dehydrogenation process at high temperatures. Given substrate is ethane and this ethane molecule heated at high temperature (750⁰ C) to produce ethylene and hydrogen gas.

To give: the reason for high temperatures needed for the dehydrogenation process.

Given reaction is favorable when ΔG is negative and change in enthalpy is positive for this reaction because two sigma bonds are braking to form one pi-bond. In addition, change in entropy is positive because one molecule is converting into two molecules. So depending on these conditions, reaction temperature should be high then only ΔG will be negative to feasible this reaction.

ΔG = ΔH-TΔSΔH = -ve ΔS = +ve

At higher temperature condition, the given reaction is feasible since ΔG is negative.

Conclusion

Conclusion

At higher temperature conditions, value of free energy will be negative so the dehydrogenation reaction is feasible at higher temperature conditions.

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

Answer 4

Question

Chapter 9, Problem 48PP

Interpretation Introduction

Interpretation:

Temperature condition is needed to be explained in the given dehydrogenation reaction.

Concept introduction:

Dehydrogenation: dehydrogenation is a process of elimination of hydrogen molecule from the substrate at high temperature condition.

Free energy: reaction is feasible when free energy is negative.

ΔG = ΔH-TΔSΔG = free energyΔH = change in enthalpyΔS = change in entropy

Expert Solution & Answer

Answer to Problem 48PP

Reaction is feasible at higher temperature conditions only since ΔG is negative at higher temperatures. Therefore, higher temperatures are needed for dehydrogenation process.

Explanation of Solution

To explain: the conditions for the given reaction.

Given reaction is shown below.

ORGANIC CHEMISTRY GGC>CUSTOM<-TEXT, Chapter 9, Problem 48PP

Clear from the reaction that the ethane molecule converted ethylene molecule at high temperature condition by releasing hydrogen gas.

Given reaction refers the dehydrogenation process at high temperatures. Given substrate is ethane and this ethane molecule heated at high temperature (750⁰ C) to produce ethylene and hydrogen gas.

To give: the reason for high temperatures needed for the dehydrogenation process.

Given reaction is favorable when ΔG is negative and change in enthalpy is positive for this reaction because two sigma bonds are braking to form one pi-bond. In addition, change in entropy is positive because one molecule is converting into two molecules. So depending on these conditions, reaction temperature should be high then only ΔG will be negative to feasible this reaction.

ΔG = ΔH-TΔSΔH = -ve ΔS = +ve

At higher temperature condition, the given reaction is feasible since ΔG is negative.

Conclusion

Conclusion

At higher temperature conditions, value of free energy will be negative so the dehydrogenation reaction is feasible at higher temperature conditions.

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

Chapter 9, Problem 48PP

Interpretation Introduction

Interpretation:

Temperature condition is needed to be explained in the given dehydrogenation reaction.

Concept introduction:

Dehydrogenation: dehydrogenation is a process of elimination of hydrogen molecule from the substrate at high temperature condition.

Free energy: reaction is feasible when free energy is negative.

ΔG = ΔH-TΔSΔG = free energyΔH = change in enthalpyΔS = change in entropy

Expert Solution & Answer

Answer to Problem 48PP

Reaction is feasible at higher temperature conditions only since ΔG is negative at higher temperatures. Therefore, higher temperatures are needed for dehydrogenation process.

Explanation of Solution

To explain: the conditions for the given reaction.

Given reaction is shown below.

ORGANIC CHEMISTRY GGC>CUSTOM<-TEXT, Chapter 9, Problem 48PP

Clear from the reaction that the ethane molecule converted ethylene molecule at high temperature condition by releasing hydrogen gas.

Given reaction refers the dehydrogenation process at high temperatures. Given substrate is ethane and this ethane molecule heated at high temperature (750⁰ C) to produce ethylene and hydrogen gas.

To give: the reason for high temperatures needed for the dehydrogenation process.

Given reaction is favorable when ΔG is negative and change in enthalpy is positive for this reaction because two sigma bonds are braking to form one pi-bond. In addition, change in entropy is positive because one molecule is converting into two molecules. So depending on these conditions, reaction temperature should be high then only ΔG will be negative to feasible this reaction.

ΔG = ΔH-TΔSΔH = -ve ΔS = +ve

At higher temperature condition, the given reaction is feasible since ΔG is negative.

Conclusion

Conclusion

At higher temperature conditions, value of free energy will be negative so the dehydrogenation reaction is feasible at higher temperature conditions.

Answer 6

Chapter 9, Problem 48PP

Interpretation Introduction

Interpretation:

Temperature condition is needed to be explained in the given dehydrogenation reaction.

Concept introduction:

Dehydrogenation: dehydrogenation is a process of elimination of hydrogen molecule from the substrate at high temperature condition.

Free energy: reaction is feasible when free energy is negative.

ΔG = ΔH-TΔSΔG = free energyΔH = change in enthalpyΔS = change in entropy

Expert Solution & Answer

Answer to Problem 48PP

Reaction is feasible at higher temperature conditions only since ΔG is negative at higher temperatures. Therefore, higher temperatures are needed for dehydrogenation process.

Explanation of Solution

To explain: the conditions for the given reaction.

Given reaction is shown below.

ORGANIC CHEMISTRY GGC>CUSTOM<-TEXT, Chapter 9, Problem 48PP

Clear from the reaction that the ethane molecule converted ethylene molecule at high temperature condition by releasing hydrogen gas.

Given reaction refers the dehydrogenation process at high temperatures. Given substrate is ethane and this ethane molecule heated at high temperature (750⁰ C) to produce ethylene and hydrogen gas.

To give: the reason for high temperatures needed for the dehydrogenation process.

Given reaction is favorable when ΔG is negative and change in enthalpy is positive for this reaction because two sigma bonds are braking to form one pi-bond. In addition, change in entropy is positive because one molecule is converting into two molecules. So depending on these conditions, reaction temperature should be high then only ΔG will be negative to feasible this reaction.

ΔG = ΔH-TΔSΔH = -ve ΔS = +ve

At higher temperature condition, the given reaction is feasible since ΔG is negative.

Conclusion

Conclusion

At higher temperature conditions, value of free energy will be negative so the dehydrogenation reaction is feasible at higher temperature conditions.

Answer 7

Chapter 9, Problem 48PP

Interpretation Introduction

Interpretation:

Temperature condition is needed to be explained in the given dehydrogenation reaction.

Concept introduction:

Dehydrogenation: dehydrogenation is a process of elimination of hydrogen molecule from the substrate at high temperature condition.

Free energy: reaction is feasible when free energy is negative.

ΔG = ΔH-TΔSΔG = free energyΔH = change in enthalpyΔS = change in entropy

Answer 8

Expert Solution & Answer

Answer to Problem 48PP

Reaction is feasible at higher temperature conditions only since ΔG is negative at higher temperatures. Therefore, higher temperatures are needed for dehydrogenation process.

Answer 9

Expert Solution & Answer

Answer 10

Expert Solution & Answer

Answer 11

Explanation of Solution

To explain: the conditions for the given reaction.

Given reaction is shown below.

ORGANIC CHEMISTRY GGC>CUSTOM<-TEXT, Chapter 9, Problem 48PP

Clear from the reaction that the ethane molecule converted ethylene molecule at high temperature condition by releasing hydrogen gas.

Given reaction refers the dehydrogenation process at high temperatures. Given substrate is ethane and this ethane molecule heated at high temperature (750⁰ C) to produce ethylene and hydrogen gas.

To give: the reason for high temperatures needed for the dehydrogenation process.

Given reaction is favorable when ΔG is negative and change in enthalpy is positive for this reaction because two sigma bonds are braking to form one pi-bond. In addition, change in entropy is positive because one molecule is converting into two molecules. So depending on these conditions, reaction temperature should be high then only ΔG will be negative to feasible this reaction.

ΔG = ΔH-TΔSΔH = -ve ΔS = +ve