The heat required to melt 1 mole of a solid is known as the
heat of fusion
heat of vaporization
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?
Vaporization involves the breaking of all forces between molecules.
Vaporization occurs at high temperatures.
Vaporization involves the breaking of bonds within molecules.
Vaporization increases the entropy of molecules.
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?
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]
London Dispersion forces
Label the phase change diagram at the following points.