Why octane boiling point is higher than the hexane and differences in boiling points. Introduction: Point where substance starts boiling and turns into vapor is called boiling point. Hexane is an alkane of six carbon atoms. C 6 H 14 is the chemical formula, and octane is a hydrocarbon and an alkane and its chemical formula is C 8 H 18 . The molecules that have strong bond with each other through intermolecular forces like hydrogen bond, weak London forces, covalent bonding therefore it do not achieve the kinetic energy, which is required to escape the liquid state, hence molecules with strong intermolecular forces have higher boiling point.

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Answer 1

Question

Chapter 7, Problem 7.71AP

Summary Introduction

To determine:

Why octane boiling point is higher than the hexane and differences in boiling points.

Introduction:

Point where substance starts boiling and turns into vapor is called boiling point. Hexane is an alkane of six carbon atoms. C₆H₁₄ is the chemical formula, and octane is a hydrocarbon and an alkane and its chemical formula is C₈H₁₈.

The molecules that have strong bond with each other through intermolecular forces like hydrogen bond, weak London forces, covalent bonding therefore it do not achieve the kinetic energy, which is required to escape the liquid state, hence molecules with strong intermolecular forces have higher boiling point.

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Answer 2

Question

Chapter 7, Problem 7.71AP

Summary Introduction

To determine:

Why octane boiling point is higher than the hexane and differences in boiling points.

Introduction:

Point where substance starts boiling and turns into vapor is called boiling point. Hexane is an alkane of six carbon atoms. C₆H₁₄ is the chemical formula, and octane is a hydrocarbon and an alkane and its chemical formula is C₈H₁₈.

The molecules that have strong bond with each other through intermolecular forces like hydrogen bond, weak London forces, covalent bonding therefore it do not achieve the kinetic energy, which is required to escape the liquid state, hence molecules with strong intermolecular forces have higher boiling point.

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Answer 3

Question

Chapter 7, Problem 7.71AP

Summary Introduction

To determine:

Why octane boiling point is higher than the hexane and differences in boiling points.

Introduction:

Point where substance starts boiling and turns into vapor is called boiling point. Hexane is an alkane of six carbon atoms. C₆H₁₄ is the chemical formula, and octane is a hydrocarbon and an alkane and its chemical formula is C₈H₁₈.

The molecules that have strong bond with each other through intermolecular forces like hydrogen bond, weak London forces, covalent bonding therefore it do not achieve the kinetic energy, which is required to escape the liquid state, hence molecules with strong intermolecular forces have higher boiling point.

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Answer 4

Question

Chapter 7, Problem 7.71AP

Summary Introduction

To determine:

Why octane boiling point is higher than the hexane and differences in boiling points.

Introduction:

Point where substance starts boiling and turns into vapor is called boiling point. Hexane is an alkane of six carbon atoms. C₆H₁₄ is the chemical formula, and octane is a hydrocarbon and an alkane and its chemical formula is C₈H₁₈.

The molecules that have strong bond with each other through intermolecular forces like hydrogen bond, weak London forces, covalent bonding therefore it do not achieve the kinetic energy, which is required to escape the liquid state, hence molecules with strong intermolecular forces have higher boiling point.

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Answer 5

Chapter 7, Problem 7.71AP

Summary Introduction

To determine:

Why octane boiling point is higher than the hexane and differences in boiling points.

Introduction:

Point where substance starts boiling and turns into vapor is called boiling point. Hexane is an alkane of six carbon atoms. C₆H₁₄ is the chemical formula, and octane is a hydrocarbon and an alkane and its chemical formula is C₈H₁₈.

The molecules that have strong bond with each other through intermolecular forces like hydrogen bond, weak London forces, covalent bonding therefore it do not achieve the kinetic energy, which is required to escape the liquid state, hence molecules with strong intermolecular forces have higher boiling point.

Answer 6

Chapter 7, Problem 7.71AP

Summary Introduction

To determine:

Why octane boiling point is higher than the hexane and differences in boiling points.

Introduction:

Point where substance starts boiling and turns into vapor is called boiling point. Hexane is an alkane of six carbon atoms. C₆H₁₄ is the chemical formula, and octane is a hydrocarbon and an alkane and its chemical formula is C₈H₁₈.

The molecules that have strong bond with each other through intermolecular forces like hydrogen bond, weak London forces, covalent bonding therefore it do not achieve the kinetic energy, which is required to escape the liquid state, hence molecules with strong intermolecular forces have higher boiling point.

Answer 7

Chapter 7, Problem 7.71AP

Summary Introduction

To determine:

Why octane boiling point is higher than the hexane and differences in boiling points.

Introduction:

Point where substance starts boiling and turns into vapor is called boiling point. Hexane is an alkane of six carbon atoms. C₆H₁₄ is the chemical formula, and octane is a hydrocarbon and an alkane and its chemical formula is C₈H₁₈.

The molecules that have strong bond with each other through intermolecular forces like hydrogen bond, weak London forces, covalent bonding therefore it do not achieve the kinetic energy, which is required to escape the liquid state, hence molecules with strong intermolecular forces have higher boiling point.

Answer 8

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Answer 9

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Answer 10

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Answer 11

Ch. 7 - Prob. 7.1PP Ch. 7 - Prob. 7.2PP Ch. 7 - Prob. 7.3PP Ch. 7 - Given that only polar molecules can participate as...Ch. 7 - Prob. 7.5PP Ch. 7 - Prob. 7.6PP Ch. 7 - An ion-dipole attraction often occurs when ionic...Ch. 7 - Prob. 7.8PP Ch. 7 - Prob. 7.9PP Ch. 7 - Prob. 7.10PP

Solution Summary: The author explains why octane's boiling point is higher than hexan, and the differences in boiling points.

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