Place the following compounds in order of decreasing strength of intermolecular forces. I.CH3CH2CH2CH2CH2CH3 $\quad$II.(CH3)3CCH3 $\quad$III.(CH3)3CCH2CH3

A) III > II > I B) I > III > II C) I > II > III D) II > III > I E) III > I > II A) III > II > I B) I > III > II C) I > II > III D) II > III > I E) III > I > II

Place the following substances in order of increasing boiling point. CH3CH2OH $\quad$Ar $\quad$CH3OCH3

A) Ar 3OCH3 3CH2OH B) CH3CH2OH 3OCH3 C) CH3CH2OH 3OCH3 3OCH3 3CH2OH E) Ar 3CH2OH 3OCH3 A) Ar 3OCH3 3CH2OH B) CH3CH2OH 3OCH3 C) CH3CH2OH 3OCH3 3OCH3 3CH2OH E) Ar 3CH2OH 3OCH3

How much energy is required to vaporize 158 g of butane (C4H10)at its boiling point if its ΔvapH is 24.3 kJ mol-1?

A) 15.1 kJ B) 66.1 kJ C) 89.4 kJ D) 11.2 kJ E) 38.4 kJ A) 15.1 kJ B) 66.1 kJ C) 89.4 kJ D) 11.2 kJ E) 38.4 kJ

How much energy is required to vaporize 48.7 g of dichloromethane (CH2Cl2)at its boiling point if its ΔvapH is 31.6 kJ mol-1?

A) 31.2 kJ B) 6.49 kJ C) 55.1 kJ D) 15.4 kJ E) 18.1 kJ A) 31.2 kJ B) 6.49 kJ C) 55.1 kJ D) 15.4 kJ E) 18.1 kJ

Exam 11: Liquids, solids, and Intermolecular Forces

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Place the following compounds in order of decreasing strength of intermolecular forces. I.CH₃CH₂CH₂CH₂CH₂CH₃ $\quad$ II.(CH₃)₃CCH₃ $\quad$ III.(CH₃)₃CCH₂CH₃

(Multiple Choice)

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Question 81

At atmospheric pressure,dry ice ________.

(Multiple Choice)

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Question 82

Give the edge length in terms of r for a simple cubic cell.

(Short Answer)

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Question 83

NaCl crystallizes in a cubic unit cell with Cl^- ions on each corner and each face.How many Na⁺ and Cl^- ions are in each unit cell of NaCl?

(Multiple Choice)

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Question 84

Identify the compound that does not have hydrogen bonding.

(Multiple Choice)

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Question 85

Describe the difference between the conduction band and the valence band.

(Essay)

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Question 86

The normal boiling point of water is ________.

(Multiple Choice)

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Question 87

Choose the substance with the highest vapour pressure at a given temperature.

(Multiple Choice)

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Question 88

What is the strongest type of intermolecular force present in H₂?

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Question 89

Ethanol ( C₂H₅OH)melts at -114 °C.The enthalpy of fusion is 5.02 kJ mol^-1.The specific heats of solid and liquid ethanol are 0.97 J g^-1 °C^-1 and 2.3 J g^-1 °C^-1,respectively.How much heat (kJ)is needed to convert 25.0 g of solid ethanol at -145 °C to liquid ethanol at -60 °C?

(Multiple Choice)

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Question 90

Place the following substances in order of increasing boiling point. CH₃CH₂OH $\quad$ Ar $\quad$ CH₃OCH₃

(Multiple Choice)

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Question 91

Choose the pair of substances that are most likely to form a homogeneous solution.

(Multiple Choice)

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Question 92

Identify the term used to describe the ability of a liquid to flow against gravity up a narrow tube.

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Question 93

Which of the following substances would you predict to have the highest Δ_vapH?

(Multiple Choice)

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Question 94

How much energy is required to vaporize 158 g of butane (C₄H₁₀)at its boiling point if its Δ_vapH is 24.3 kJ mol^-1?

(Multiple Choice)

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Question 95

Identify the compound that does not have dipole-dipole forces as its strongest force.

(Multiple Choice)

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Question 96

Choose the pair of substances that are most likely to form a homogeneous solution.

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Question 97

Which one of the following has a definite shape and volume?

(Multiple Choice)

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Question 98

How much energy is required to vaporize 48.7 g of dichloromethane (CH₂Cl₂)at its boiling point if its Δ_vapH is 31.6 kJ mol^-1?

(Multiple Choice)

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Question 99

Choose the molecule or compound that exhibits dispersion forces as its strongest intermolecular force.

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Question 100

Showing 81 - 100 of 127

Exam 11: Liquids, solids, and Intermolecular Forces

Place the following compounds in order of decreasing strength of intermolecular forces. I.CH3CH2CH2CH2CH2CH3 \quad II.(CH3)3CCH3 \quad III.(CH3)3CCH2CH3

At atmospheric pressure,dry ice ________.

Give the edge length in terms of r for a simple cubic cell.

NaCl crystallizes in a cubic unit cell with Cl- ions on each corner and each face.How many Na+ and Cl- ions are in each unit cell of NaCl?

Identify the compound that does not have hydrogen bonding.

Describe the difference between the conduction band and the valence band.

The normal boiling point of water is ________.

Choose the substance with the highest vapour pressure at a given temperature.

What is the strongest type of intermolecular force present in H2?

Ethanol ( C2H5OH)melts at -114 °C.The enthalpy of fusion is 5.02 kJ mol-1.The specific heats of solid and liquid ethanol are 0.97 J g-1 °C-1 and 2.3 J g-1 °C-1,respectively.How much heat (kJ)is needed to convert 25.0 g of solid ethanol at -145 °C to liquid ethanol at -60 °C?

Place the following substances in order of increasing boiling point. CH3CH2OH \quad Ar \quad CH3OCH3

Choose the pair of substances that are most likely to form a homogeneous solution.

Identify the term used to describe the ability of a liquid to flow against gravity up a narrow tube.

Which of the following substances would you predict to have the highest ΔvapH?

How much energy is required to vaporize 158 g of butane (C4H10)at its boiling point if its ΔvapH is 24.3 kJ mol-1?

Identify the compound that does not have dipole-dipole forces as its strongest force.

Choose the pair of substances that are most likely to form a homogeneous solution.

Which one of the following has a definite shape and volume?

How much energy is required to vaporize 48.7 g of dichloromethane (CH2Cl2)at its boiling point if its ΔvapH is 31.6 kJ mol-1?

Choose the molecule or compound that exhibits dispersion forces as its strongest intermolecular force.

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Place the following compounds in order of decreasing strength of intermolecular forces. I.CH₃CH₂CH₂CH₂CH₂CH₃ $\quad$ II.(CH₃)₃CCH₃ $\quad$ III.(CH₃)₃CCH₂CH₃

NaCl crystallizes in a cubic unit cell with Cl^- ions on each corner and each face.How many Na⁺ and Cl^- ions are in each unit cell of NaCl?

What is the strongest type of intermolecular force present in H₂?

Ethanol ( C₂H₅OH)melts at -114 °C.The enthalpy of fusion is 5.02 kJ mol^-1.The specific heats of solid and liquid ethanol are 0.97 J g^-1 °C^-1 and 2.3 J g^-1 °C^-1,respectively.How much heat (kJ)is needed to convert 25.0 g of solid ethanol at -145 °C to liquid ethanol at -60 °C?

Place the following substances in order of increasing boiling point. CH₃CH₂OH $\quad$ Ar $\quad$ CH₃OCH₃

Which of the following substances would you predict to have the highest Δ_vapH?

How much energy is required to vaporize 158 g of butane (C₄H₁₀)at its boiling point if its Δ_vapH is 24.3 kJ mol^-1?

How much energy is required to vaporize 48.7 g of dichloromethane (CH₂Cl₂)at its boiling point if its Δ_vapH is 31.6 kJ mol^-1?