Question 1

Vanadium crystallizes in a body-centered cubic lattice, and the length of the edge of a unit cell is 305 pm. What is the density of V

Accepted Answer

A)  5.96 * 10-30 g/cm3 
B)  2.98 * 10-6 g/cm3 
C)  2.98 g/cm3 
D)  5.96 g/cm3 
E)  11.9 g/cm3 
A)  5.96 * 10-30 g/cm3 
B)  2.98 * 10-6 g/cm3 
C)  2.98 g/cm3 
D)  5.96 g/cm3 
E)  11.9 g/cm3

Question 2

The freezing point of a liquid does not change as the atmospheric pressure changes.

Accepted Answer

A) True 
 B)False

Question 3

Which of the following liquids would have the lowest viscosity at 25$\circ$C

Accepted Answer

A)  A 
B)  B 
C)  C 
D)  D 
E)  E 
A)  A 
B)  B 
C)  C 
D)  D 
E)  E

Question 4

HOCH2CH2OH(s) is classified as a/an

Accepted Answer

A)  metallic crystal. 
B)  covalent solid. 
C)  molecular crystal. 
D)  amorphous solid. 
E)  ionic crystal. 
A)  metallic crystal. 
B)  covalent solid. 
C)  molecular crystal. 
D)  amorphous solid. 
E)  ionic crystal.

Question 5

How much energy (heat) is required to convert 25.5 g of H2O(l) at 35.0$\circ$C to H2O(g) at 115.0$\circ$C

specific heat of ice: $ \quad 2.09 \mathrm{~J} / \mathrm{g} \cdot{ }^{\circ} \mathrm{C} \quad \Delta \mathrm{H}_{\mathrm{fus}}=6.02 \mathrm{~kJ} / \mathrm{mol} $ 
specific heat of water: $ 4.18 \mathrm{~J} / \mathrm{g}{ \cdot}^{\circ} \mathrm{C} \quad \Delta \mathrm{H}_{\mathrm{vap}}=40.7 \mathrm{~kJ} / \mathrm{mo} $. 
specific hast of steam: $ 1.84 \mathrm{~J} / \mathrm{g} \cdot{ }^{\circ} \mathrm{C} $

Accepted Answer

A)  207 J 
B)  7,630 J 
C)  8,530 J 
D)  9,130 J 
E)  65,200 J 
A)  207 J 
B)  7,630 J 
C)  8,530 J 
D)  9,130 J 
E)  65,200 J

Question 6

C8H18 has a higher vapor pressure than C4H10.

Accepted Answer

A) True 
 B)False

Question 7

Octane, C8H18, boils at 125$\circ$C as compared to water, which boils at 100$\circ$C. This information suggests that the dispersion forces in nonpolar octane molecules are stronger than dispersion forces and hydrogen bonding in water.

Accepted Answer

A) True 
 B)False

Question 8

NH3 has a higher boiling point than PH3.

Accepted Answer

A) True 
 B)False

Question 9

Which of the following constants is/are needed to calculate the amount of energy required to heat 30.5g of H2O(s) at -25.0$\circ$C to H2O(l) at 55.0$\circ$C
I. $\Delta$Hfus (H2O)
II. $\Delta$Hvap (H2O)
III. specific heat of H2O(s)
IV. specific heat of H2O(l)
V. specific heat of H2O(g)

Accepted Answer

A)  I, II, III, IV, and IV 
B)  I, III, and IV 
C)  III and IV 
D)  I only 
E)  I, II, III, and IV 
A)  I, II, III, IV, and IV 
B)  I, III, and IV 
C)  III and IV 
D)  I only 
E)  I, II, III, and IV

Question 10

Use the graph of vapor pressure to determine the normal boiling point of CHCl3.

Accepted Answer

A)  19$\circ$C 
B)  52$\circ$C 
C)  60$\circ$C 
D)  64$\circ$C 
E)  70$\circ$C 
A)  19$\circ$C 
B)  52$\circ$C 
C)  60$\circ$C 
D)  64$\circ$C 
E)  70$\circ$C

Question 11

CH4 has a higher boiling point than CH3OH.

Accepted Answer

A) True 
 B)False

Question 12

Acetic acid has a heat of fusion of 10.8 kJ/mol and a heat of vaporization of 24.3 kJ/mol. What is the expected value for the heat of sublimation of acetic acid

Accepted Answer

A)  35.1 kJ/mol 
B)  -13.5 kJ/mol 
C)  +13.5 kJ/mol 
D)  -35.1 kJ/mol 
E)  Not enough information is given to answer the question. 
A)  35.1 kJ/mol 
B)  -13.5 kJ/mol 
C)  +13.5 kJ/mol 
D)  -35.1 kJ/mol 
E)  Not enough information is given to answer the question.

Question 13

C(CH3)4 has a higher vapor pressure than CH3CH2CH2CH2CH3.

Accepted Answer

A) True 
 B)False

Question 14

Which one of the following substances should exhibit hydrogen bonding in the liquid state

Accepted Answer

A)  SiH4 
B)  H2 
C)  H2S 
D)  CH4 
E)  CH3NH2 
A)  SiH4 
B)  H2 
C)  H2S 
D)  CH4 
E)  CH3NH2

Question 15

Which one of the following substances is expected to have the highest boiling point

Accepted Answer

A)  HBr 
B)  HCl 
C)  HF 
D)  HI 
A)  HBr 
B)  HCl 
C)  HF 
D)  HI

Question 16

Find the temperature at which water boils on a day in the mountains when the barometric pressure is 593 mmHg. (Given: the heat of vaporization of water is 40.79 kJ/mol)

Accepted Answer

A)  41.5$\circ$C 
B)  68.1$\circ$C 
C)  93.1$\circ$C 
D)  97.0$\circ$C 
E)  117$\circ$C 
A)  41.5$\circ$C 
B)  68.1$\circ$C 
C)  93.1$\circ$C 
D)  97.0$\circ$C 
E)  117$\circ$C

Question 17

3.59 g of water was introduced into an evacuated 1.50 L flask at 30$\circ$C. What mass of water will evaporate (Vapor pressure of water at 30$\circ$C is 31.82 mmHg.)

Accepted Answer

A)  2.52 * 10-3 g 
B)  0.04187 g 
C)  0.0455g 
D)  0.4187 g 
E)  0.455 g 
A)  2.52 * 10-3 g 
B)  0.04187 g 
C)  0.0455g 
D)  0.4187 g 
E)  0.455 g

Question 18

Find the temperature at which ethanol boils on a day in the mountains when the barometric pressure is 547 mmHg. (Given: The heat of vaporization of ethanol is 39.3 kJ/mol; the normal boiling point of ethanol is 78.3$\circ$C.)

Accepted Answer

A)  10.0$\circ$C 
B)  69.9$\circ$C 
C)  74.6$\circ$C 
D)  76.5$\circ$C 
E)  77.9$\circ$C 
A)  10.0$\circ$C 
B)  69.9$\circ$C 
C)  74.6$\circ$C 
D)  76.5$\circ$C 
E)  77.9$\circ$C

Question 19

Solid iodine has a vapor pressure of 1.0 mmHg at 39$\circ$C. How many moles of iodine will sublime into a 500 mL flask at this temperature If the volume of the flask is doubled at constant temperature, what will happen to the equilibrium vapor pressure of I2
(Assume some solid I2 is always present in the container.)

Accepted Answer

A)  2.1 * 10-4 mol; vapor pressure increases 
B)  2.0 * 10-2 mol; vapor pressure increases 
C)  2.6 * 10-5 mol; no change in vapor pressure 
D)  2.1 * 10-4 mol; no change in vapor pressure 
E)  2.6 * 10-5 mol; vapor pressure decreases 
A)  2.1 * 10-4 mol; vapor pressure increases 
B)  2.0 * 10-2 mol; vapor pressure increases 
C)  2.6 * 10-5 mol; no change in vapor pressure 
D)  2.1 * 10-4 mol; no change in vapor pressure 
E)  2.6 * 10-5 mol; vapor pressure decreases

Question 20

Platinum has a face-centered cubic crystal structure and a density of 21.5 g/cm3. What is the radius of the platinum atom

Accepted Answer

A)  69 pm 
B)  98 pm 
C)  139 pm 
D)  196 pm 
E)  277 pm 
A)  69 pm 
B)  98 pm 
C)  139 pm 
D)  196 pm 
E)  277 pm

Exam 11: Intermolecular Forces and Liquids and Solids

Vanadium crystallizes in a body-centered cubic lattice, and the length of the edge of a unit cell is 305 pm. What is the density of V

The freezing point of a liquid does not change as the atmospheric pressure changes.

Which of the following liquids would have the lowest viscosity at 25 ∘\circ∘ C

HOCH2CH2OH(s) is classified as a/an

C8H18 has a higher vapor pressure than C4H10.

Octane, C8H18, boils at 125 ∘\circ∘ C as compared to water, which boils at 100 ∘\circ∘ C. This information suggests that the dispersion forces in nonpolar octane molecules are stronger than dispersion forces and hydrogen bonding in water.

NH3 has a higher boiling point than PH3.

Use the graph of vapor pressure to determine the normal boiling point of CHCl3.

CH4 has a higher boiling point than CH3OH.

Acetic acid has a heat of fusion of 10.8 kJ/mol and a heat of vaporization of 24.3 kJ/mol. What is the expected value for the heat of sublimation of acetic acid

C(CH3)4 has a higher vapor pressure than CH3CH2CH2CH2CH3.

Which one of the following substances should exhibit hydrogen bonding in the liquid state

Which one of the following substances is expected to have the highest boiling point

Find the temperature at which water boils on a day in the mountains when the barometric pressure is 593 mmHg. (Given: the heat of vaporization of water is 40.79 kJ/mol)

3.59 g of water was introduced into an evacuated 1.50 L flask at 30 ∘\circ∘ C. What mass of water will evaporate (Vapor pressure of water at 30 ∘\circ∘ C is 31.82 mmHg.)

Find the temperature at which ethanol boils on a day in the mountains when the barometric pressure is 547 mmHg. (Given: The heat of vaporization of ethanol is 39.3 kJ/mol; the normal boiling point of ethanol is 78.3 ∘\circ∘ C.)

Platinum has a face-centered cubic crystal structure and a density of 21.5 g/cm3. What is the radius of the platinum atom

Chemistry: The Study of Change

Atoms Molecules and Ions

Mass Relationships in Chemical Reactions

Reactions in Aqueous Solutions

Gases

Thermochemistry

Quantum Theory and the Electronic Structure of Atoms

Periodic Relationships Among the Elements

Chemical Bonding I: Basic Concepts

Chemical Bonding II: Molecular Geometry and Hybridization of Atomic

Physical Properties of Solutions

Chemical Kinetics

Chemical Equilibrium

Acids and Bases

Acid-Base Equilibria and Solubility Equilibria

Entropy Free Energy and Equilibrium

Electrochemistry

Nuclear Chemistry

Chemistry in the Atmosphere

Metallurgy and the Chemistry of Metals

Nonmetallic Elements and Their Compounds

Transition Metals Chemistry and Coordination Compounds

Organic Chemistry

Synthetic and Natural Organic Polymers

Filters

Which of the following liquids would have the lowest viscosity at 25^$\circ$C $Which of the following liquids would have the lowest viscosity at 25<sup> \circ </sup>C$

HOCH₂CH₂OH(s) is classified as a/an

C₈H₁₈ has a higher vapor pressure than C₄H₁₀.

Octane, C₈H₁₈, boils at 125^$\circ$C as compared to water, which boils at 100^$\circ$C. This information suggests that the dispersion forces in nonpolar octane molecules are stronger than dispersion forces and hydrogen bonding in water.

NH₃ has a higher boiling point than PH₃.

Use the graph of vapor pressure to determine the normal boiling point of CHCl₃.

CH₄ has a higher boiling point than CH₃OH.

C(CH₃)₄ has a higher vapor pressure than CH₃CH₂CH₂CH₂CH₃.

3.59 g of water was introduced into an evacuated 1.50 L flask at 30^$\circ$C. What mass of water will evaporate (Vapor pressure of water at 30^$\circ$C is 31.82 mmHg.)

Find the temperature at which ethanol boils on a day in the mountains when the barometric pressure is 547 mmHg. (Given: The heat of vaporization of ethanol is 39.3 kJ/mol; the normal boiling point of ethanol is 78.3^$\circ$C.)

Platinum has a face-centered cubic crystal structure and a density of 21.5 g/cm³. What is the radius of the platinum atom