Question 1

Calculate the amount of heat needed to melt 2.00 kg of iron at its melting point (1,809 K), given that $\Delta$Hfus = 13.80 kJ/mol.

Accepted Answer

A)  27,600 J 
B)  27.6 kJ 
C)  494 kJ 
D)  25,000 kJ 
E)  27,600 kJ 
A)  27,600 J 
B)  27.6 kJ 
C)  494 kJ 
D)  25,000 kJ 
E)  27,600 kJ

Question 2

Which property of water allows a razor blade to float on it without sinking

Accepted Answer

A)  viscosity 
B)  surface tension 
C)  density 
D)  specific heat 
E)  triple point 
A)  viscosity 
B)  surface tension 
C)  density 
D)  specific heat 
E)  triple point

Question 3

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

Accepted Answer

A)  CH3OCH3 
B)  CH2Cl2 
C)  C2H5OH 
D)  CH3Br 
E)  HOCH2CH2OH 
A)  CH3OCH3 
B)  CH2Cl2 
C)  C2H5OH 
D)  CH3Br 
E)  HOCH2CH2OH

Question 4

The gas phase exists at the point labeled c.

Accepted Answer

A) True 
 B)False

Question 5

For which of the following species are the dispersion forces strongest

Accepted Answer

A)  C4H10 
B)  C5H12 
C)  C6H14 
D)  C7H16 
E)  C8H18 
A)  C4H10 
B)  C5H12 
C)  C6H14 
D)  C7H16 
E)  C8H18

Question 6

The triple point of iodine is at 0.12 atm and 115$\circ$C. Thus, liquid I2

Accepted Answer

A)  is more dense than I2 (s). 
B)  cannot exist above 115$\circ$C. 
C)  is liquid at room temperature. 
D)  cannot have a vapor pressure less than 91 torr. 
A)  is more dense than I2 (s). 
B)  cannot exist above 115$\circ$C. 
C)  is liquid at room temperature. 
D)  cannot have a vapor pressure less than 91 torr.

Question 7

Which of the following constants is/are needed to calculate the amount of energy required to heat 12.0g of H2O(l) at 30.0$\circ$C to H2O(l) at 85.0$\circ$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 and IV 
B)  II and IV 
C)  IV only 
D)  I, II, and IV 
E)  IV and V 
A)  I and IV 
B)  II and IV 
C)  IV only 
D)  I, II, and IV 
E)  IV and V

Question 8

The number of atoms in a face-centered cubic unit cell is

Accepted Answer

A)  1 
B)  2 
C)  3 
D)  4 
E)  8 
A)  1 
B)  2 
C)  3 
D)  4 
E)  8

Question 9

The boiling points of chloromethane (CH3Cl) and dichlormethane (CH2Cl2) are - 24 $\circ$C and 40.$\circ$C respectively. The boiling point of trichloromethane (CHCl3) is predicted to be:

Accepted Answer

A)  $\circ$C 
B)  > 40.$\circ$C 
C)  > - 24 $\circ$C and $\circ$C 
D)  - 24 $\circ$C 
E)  40.$\circ$C 
A)  $\circ$C 
B)  > 40.$\circ$C 
C)  > - 24 $\circ$C and $\circ$C 
D)  - 24 $\circ$C 
E)  40.$\circ$C

Question 10

Use the following data to determine the molar heat of vaporization of chlorine. $\begin{array}{llll} 
T(^\circ{C})\
& -84.5 & -71.2 & -47.3 \
P(\mathrm{mmHg})~~~~ & & &\
&40.0&100.0&400.0
\end{array}$

Accepted Answer

A)  34,700 J 
B)  21,900 J 
C)  9.99 kJ 
D)  712 J 
E)  317 J 
A)  34,700 J 
B)  21,900 J 
C)  9.99 kJ 
D)  712 J 
E)  317 J

Question 11

The heat capacity of liquid water is 4.18 J/g·$\circ$C and the heat of vaporization is 40.7 kJ/mol. How many kilojoules of heat must be provided to convert 1.00 g of liquid water at 67$\circ$C into 1.00 g of steam at 100$\circ$C

Accepted Answer

A)  40.8 J 
B)  2.2 kJ 
C)  2,400 J 
D)  22.7 kJ 
E)  40.8 kJ 
A)  40.8 J 
B)  2.2 kJ 
C)  2,400 J 
D)  22.7 kJ 
E)  40.8 kJ

Question 12

The boiling points of propanol (CH3CH2CH2OH) and pentanol (CH3CH2CH2CH2CH2OH) are 97$\circ$C and 137$\circ$C, respectively. The boiling point of butanol (CH3CH2CH2CH2OH) is predicted to be:

Accepted Answer

A)  $\circ$C 
B)  > 137$\circ$C 
C)  > 97$\circ$C and $\circ$C 
D)  97$\circ$C 
E)  137$\circ$C 
A)  $\circ$C 
B)  > 137$\circ$C 
C)  > 97$\circ$C and $\circ$C 
D)  97$\circ$C 
E)  137$\circ$C

Question 13

Each of the following substances is a liquid at -50$\circ$C. Place these liquids in order of increasing vapor pressure: dimethyl ether (CH3OCH3), propane (C3H8), and ethanol (CH3CH2OH).

Accepted Answer

A)  ethanol < propane < dimethyl ether 
B)  ethanol < dimethyl ether < propane 
C)  propane < dimethyl ether < ethanol 
D)  dimethyl ether < ethanol < propane 
E)  propane < ethanol < dimethyl ether 
A)  ethanol < propane < dimethyl ether 
B)  ethanol < dimethyl ether < propane 
C)  propane < dimethyl ether < ethanol 
D)  dimethyl ether < ethanol < propane 
E)  propane < ethanol < dimethyl ether

Question 14

The molar heats of sublimation and fusion of iodine are 62.3 kJ/mol and15.3 kJ/mol, respectively. Calculate the molar heat of vaporization of liquid iodine.

Accepted Answer

A)  -77.6 kJ/mol 
B)  47.0 kJ/mol 
C)  -47.0 kJ/mol 
D)  77.6 kJ/mol 
E)  4.07 kJ/mol 
A)  -77.6 kJ/mol 
B)  47.0 kJ/mol 
C)  -47.0 kJ/mol 
D)  77.6 kJ/mol 
E)  4.07 kJ/mol

Question 15

CH3Cl has a higher boiling point than CH4.

Accepted Answer

A) True 
 B)False

Question 16

HF has stronger intermolecular forces of attraction than HCl.

Accepted Answer

A) True 
 B)False

Question 17

Given that the heat of vaporization of diethyl ether is 26.0 kJ/mol and the vapor pressure of diethyl ether is 440 torr at 20.$\circ$C, calculate the normal boiling point of diethyl ether.

Accepted Answer

A)  38$\circ$C 
B)  36$\circ$C 
C)  34$\circ$C 
D)  32$\circ$C 
E)  None of the above 
A)  38$\circ$C 
B)  36$\circ$C 
C)  34$\circ$C 
D)  32$\circ$C 
E)  None of the above

Question 18

Boron nitride, BN3, melts at approximately at 3,000$\circ$C under high pressure. This material is almost as hard as diamond. What kind of crystal is this

Accepted Answer

A)  Ionic Crystal 
B)  Covalent Crystal 
C)  Metallic Crystal 
D)  Molecular Crystal 
E)  Amorphous (Not a regular crystal) 
A)  Ionic Crystal 
B)  Covalent Crystal 
C)  Metallic Crystal 
D)  Molecular Crystal 
E)  Amorphous (Not a regular crystal)

Question 19

The number of atoms in a body-centered cubic unit cell is

Accepted Answer

A)  1 
B)  2 
C)  3 
D)  4 
E)  8 
A)  1 
B)  2 
C)  3 
D)  4 
E)  8

Question 20

All intermolecular forces must be overcome in order for a substance to undergo a phase change from a liquid to a gas

Accepted Answer

A) True 
 B)False

Exam 11: Intermolecular Forces and Liquids and Solids

Calculate the amount of heat needed to melt 2.00 kg of iron at its melting point (1,809 K), given that Δ\DeltaΔ Hfus = 13.80 kJ/mol.

Which property of water allows a razor blade to float on it without sinking

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

The gas phase exists at the point labeled c.

For which of the following species are the dispersion forces strongest

The triple point of iodine is at 0.12 atm and 115 ∘\circ∘ C. Thus, liquid I2

The number of atoms in a face-centered cubic unit cell is

The boiling points of chloromethane (CH3Cl) and dichlormethane (CH2Cl2) are - 24 ∘\circ∘ C and 40. ∘\circ∘ C respectively. The boiling point of trichloromethane (CHCl3) is predicted to be:

Use the following data to determine the molar heat of vaporization of chlorine. T C ) -84.5 -71.2 -47.3 P()\nobreakspace\nobreakspace\nobreakspace\nobreakspace 40.0 100.0 400.0

The heat capacity of liquid water is 4.18 J/g· ∘\circ∘ C and the heat of vaporization is 40.7 kJ/mol. How many kilojoules of heat must be provided to convert 1.00 g of liquid water at 67 ∘\circ∘ C into 1.00 g of steam at 100 ∘\circ∘ C

The boiling points of propanol (CH3CH2CH2OH) and pentanol (CH3CH2CH2CH2CH2OH) are 97 ∘\circ∘ C and 137 ∘\circ∘ C, respectively. The boiling point of butanol (CH3CH2CH2CH2OH) is predicted to be:

Each of the following substances is a liquid at -50 ∘\circ∘ C. Place these liquids in order of increasing vapor pressure: dimethyl ether (CH3OCH3), propane (C3H8), and ethanol (CH3CH2OH).

The molar heats of sublimation and fusion of iodine are 62.3 kJ/mol and15.3 kJ/mol, respectively. Calculate the molar heat of vaporization of liquid iodine.

CH3Cl has a higher boiling point than CH4.

HF has stronger intermolecular forces of attraction than HCl.

Given that the heat of vaporization of diethyl ether is 26.0 kJ/mol and the vapor pressure of diethyl ether is 440 torr at 20. ∘\circ∘ C, calculate the normal boiling point of diethyl ether.

Boron nitride, BN3, melts at approximately at 3,000 ∘\circ∘ C under high pressure. This material is almost as hard as diamond. What kind of crystal is this

The number of atoms in a body-centered cubic unit cell is

All intermolecular forces must be overcome in order for a substance to undergo a phase change from a liquid to a gas

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Calculate the amount of heat needed to melt 2.00 kg of iron at its melting point (1,809 K), given that $\Delta$ H_fus = 13.80 kJ/mol.

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

The triple point of iodine is at 0.12 atm and 115^$\circ$C. Thus, liquid I₂

The boiling points of chloromethane (CH₃Cl) and dichlormethane (CH₂Cl₂) are - 24 ^$\circ$C and 40.^$\circ$C respectively. The boiling point of trichloromethane (CHCl₃) is predicted to be:

The heat capacity of liquid water is 4.18 J/g·^$\circ$C and the heat of vaporization is 40.7 kJ/mol. How many kilojoules of heat must be provided to convert 1.00 g of liquid water at 67^$\circ$C into 1.00 g of steam at 100^$\circ$C

The boiling points of propanol (CH₃CH₂CH₂OH) and pentanol (CH₃CH₂CH₂CH₂CH₂OH) are 97^$\circ$C and 137^$\circ$C, respectively. The boiling point of butanol (CH₃CH₂CH₂CH₂OH) is predicted to be:

Each of the following substances is a liquid at -50^$\circ$C. Place these liquids in order of increasing vapor pressure: dimethyl ether (CH₃OCH₃), propane (C₃H₈), and ethanol (CH₃CH₂OH)_.

CH₃Cl has a higher boiling point than CH₄.

Given that the heat of vaporization of diethyl ether is 26.0 kJ/mol and the vapor pressure of diethyl ether is 440 torr at 20.^$\circ$C, calculate the normal boiling point of diethyl ether.

Boron nitride, BN₃, melts at approximately at 3,000^$\circ$C under high pressure. This material is almost as hard as diamond. What kind of crystal is this