Chapter 11: Liquids and Phase changes

In water, the melting point is unusually high because of

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

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?

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

Of the following _____ is an exothermic process.

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

The resistance of a liquid to flow is known as

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

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

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

Which od the following expected to have the greatest viscosity?

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

Which of the following compounds has the highest boiling point?

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

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?

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

Correctly identify the phase changes occurring in the following: Solid to liquid = [blank_start]Melting[blank_end] Liquid to gas = [blank_start]Vaporization[blank_end] Solid to gas = [blank_start]Sublimation[blank_end] Gas to liquid = [blank_start]Condensation[blank_end] Liquid to solid = [blank_start]Freezing[blank_end] Gas to solid = [blank_start]Deposition[blank_end]

Which of the following phase changes is endothermic?

Which of the following phase changes is exothermic?

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)

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)

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.

[blank_start]Dipole-diploe attraction[blank_end] --> The attraction of one polar molecule for another Example of this would be [blank_start]HCl[blank_end] [blank_start]Hydrogen bonding[blank_end] --> special dipole-dipole where the hydrogen attaches to a F, N, or O. Very strong. Example of this would be [blank_start]H2O[blank_end] [blank_start]London Dispersion forces[blank_end] --> Stronger for larger molecules, but typically weak and abundant. Example of this would be [blank_start]CH3CH2CH2CH3[blank_end]

Label the phase change diagram at the following points.

Normal melting and boiling point occur at what pressure?