Exam 11: Liquids, Solids, and Intermolecular Forces

How much energy must be removed from a 94.4 g sample of benzene (molar mass = 78.11 g mol^-1)at 322.0 K to solidify the sample and lower the temperature to 205.0 K? The following physical data may be useful: Δ_vapH = 33.9 kJ mol^-1 Δ_fusH = 9.8 kJ mol^-1 C_liq = 1.73 J g^-1 °C^-1 C_gas = 1.06 J g^-1 °C^-1 C_sol = 1.51 J g^-1 °C^-1 T_melting = 279.0 K T_boiling = 353.0 K

Define viscosity.

Gold crystallizes in a face-centred cubic structure. What is the edge length of the unit cell if the atomic radius of gold is 144 pm?

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

Define the boiling point of a liquid.

Which of the following statements is TRUE?

Define deposition.

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

Sketch the phase diagram of benzene. Make sure to label the axes and the different phases of benzene. Use the physical data provided below. melting point = 279 K boiling point = 353 K T_c = 562 K P_c = 49.0 bar Triple point = 0.05 bar, 279 K

Consider the phase diagram shown. Choose the statement below that is TRUE.

The energy required to increase the surface area of a liquid by a unit amount is called ________.

Place the following substances in order of decreasing vapour pressure at a given temperature. PF₅ BrF₃ CF₄

How much energy is required to heat 87.1 g acetone (molar mass = 58.08 g mol^-1)from a solid at -154.0 °C to a liquid at -42. 0°C? The following physical data may be useful: Δ_fusH = 7.27 kJ mol^-1 C_liq = 2.16 J g^-1 °C^-1 C_gas = 1.29 J g^-1 °C^-1 C_sol = 1.65 J g^-1 °C^-1 T_melting = -95.0 °C

Which of the following compounds exhibits hydrogen bonding?

Place the following compounds in order of increasing strength of intermolecular forces. CO₂ F₂ NH₂CH₃

The boiling point of water is ________.

Which of the following is considered an atomic solid?

Match the following. -LiI + H₂O

Why does the temperature of a substance stay constant during a phase change such as vaporization?

The enthalpy change for converting 10.0 g of ice at -25.0 °C to water at 80.0 °C is ________ kJ. The specific heats of ice, water, and steam are 2.09 J g^-1 °C^-1, 4.18 J g^-1 °C^-1, and 1.84 J g^-1 °C^-1, respectively. For H₂O, Δ_fusH = 6.01 kJ mol^-1, and Δ_vapH = 40.67 kJ mol^-1.