Chapter 11: Liquids and Phase changes

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In water, the melting point is unusually high because of

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The main interactions between molecules of hydrogen chloride are examples of ____?

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If the heat of vaporization for water is 2260 J/g, how many kilojoules are required to convert 5.00 g of liquid water at 100 °C to steam at 100 °C?

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Which of the following has dispersion forces as its only intermolecular force?

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Of the following _____ is an exothermic process.

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

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The resistance of a liquid to flow is known as

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Which one of the following substances will not have hydrogen bonding as one of its intermolecular forces?

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The heat required to melt 1 mole of a solid is known as the

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Which of the intermolecular forces is the most important contributor to the high surface tension shown by water?

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Which od the following expected to have the greatest viscosity?

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Which of the following best explains why ∆Hvap is usually higher than ∆Hfusion?

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Which of the following compounds has the highest boiling point?

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Which of the following would be expected to have the highest surface tension?

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Ethyl chloride, C2H5Cl, is used as a local anesthetic. It works by colling tissue as it vaporizes. The heat of vaporization is 26.4 kJ/mol. How much heat could be removed by 60.0 g of ethyl chloride?

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Which of the following is NOT considered a property of a liquid?

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Correctly identify the phase changes occurring in the following:
Solid to liquid = ❌
Liquid to gas = ❌
Solid to gas = ❌
Gas to liquid = ❌
Liquid to solid = ❌
Gas to solid = ❌

Melting

Vaporization

Sublimation

Condensation

Freezing

Deposition

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Which of the following phase changes is endothermic?

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Which of the following phase changes is exothermic?

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Q=MC∆T
Where Q is the specific heat
M is mass in moles
C is heat capacity
∆T is change in temperature (in celsius or kelvin)

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How much energy (kJ) is released when 15.3 grams of steam at 115.0 °C is condensed to give liquid water at 75 °C?
Hvap of liquid water is 40.67 kJ/mol
Heat capacity of liquid= 75.3 J/(K⋅mol)
Heat capacity of vapor= 33.6 J/(K⋅mol)

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How much energy in kilojoules is needed to heat 4.65 g of ice from -11.5 ∘C to 34.0 ∘C? The heat of fusion of water is 6.01 kJ/mol, and the molar heat capacity is 36.6 J/(K⋅mol) for ice and 75.4 J/(K⋅mol) for liquid water.

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❌ --> The attraction of one polar molecule for another
Example of this would be ❌
❌ --> special dipole-dipole where the hydrogen attaches to a F, N, or O. Very strong.
Example of this would be ❌
❌ --> Stronger for larger molecules, but typically weak and abundant.
Example of this would be ❌

Dipole-diploe attraction

HCl

Hydrogen bonding

H2O

London Dispersion forces

CH3CH2CH2CH3

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Label the phase change diagram at the following points.

Solid

Liquid

Gas

Triple Point

Critical point

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Normal melting and boiling point occur at what pressure?

University Chemistry 102 Quiz on Chapter 11: Liquids and Phase changes, created by Laura Pepe on 09/02/2020.