Question 1

Arrange the following substances in order of increasing boiling point: CH3CH2OH, HOCH2CH2OH, CH3CH2Cl, and ClCH2CH2OH

Accepted Answer

A) CH3CH2OH 2CH2OH 3CH2Cl 2CH2OH 
B) CH3CH2Cl 3CH2OH 2CH2OH 2CH2OH 
C) CH3CH2OH 3CH2Cl 2CH2OH 2CH2OH 
D) CH3CH2Cl 2CH2OH 3CH2OH 2CH2OH 
E) CH3CH2OH 2CH2OH 3CH2Cl 2CH2OH `

Question 2

Identify the dominant (strongest)type of intermolecular force present in Cl₂(l).

Accepted Answer

The answer of Identify the dominant (strongest)type of intermolecular force...

Question 3

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

Question 4

The specific heat of liquid ethanol, C2H5OH(l), is 2.46 J/g·°C and the heat of vaporization is 39.3 kJ/mol.The boiling point of ethanol is 78.3 °C.What amount of enthalpy is required to heat 50.0 g of liquid ethanol from 23.0 °C to ethanol vapor at 78.3 °C?

Accepted Answer

A) 42.7 kJ 
B) 49.5 kJ 
C) 179 kJ 
D) 1970kJ 
E) 6840 kJ

Question 5

Potassium crystallizes in a body-centered cubic lattice.How many atoms are there per unit cell?

Accepted Answer

A) 1 
B) 2 
C) 4 
D) 6 
E) 8

Question 6

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.

Question 7

Indicate all the types of intermolecular forces of attraction in He(l).

Accepted Answer

The answer of Indicate all the types of intermolecular forces...

Question 8

Sodium iodide, NaI, melts at 651°C.In its liquid state NaI conducts electricity.What kind of crystal is this?

Accepted Answer

The answer of Sodium iodide, NaI, melts at 651°C.In its...

Question 9

What mass of water would need to evaporate from your skin in order to dissipate 1.7 × 105 J of heat from your body? H2O(l)$\rarr$ H2O(g)$\Delta$Hvap = 40.7 kJ/mol

Accepted Answer

A) 58.4 g 
B) 75.2 g 
C) 418 g 
D) 7.52 × 104 g 
E) 6.92 × 106 g

Question 10

Identify the dominant (strongest)type of intermolecular force present in H₂S(g).

Accepted Answer

The answer of Identify the dominant (strongest)type of intermolecular force...

Question 11

An example of a covalent network solid is

Accepted Answer

A) diamond. 
B) potassium. 
C) iodine. 
D) sodium chloride. 
E) None of these.

Question 12

Which of the following phase changes is exothermic?

Accepted Answer

A) Sublimation 
B) Condensation 
C) Melting 
D) Vaporization

Question 13

Calculate the amount of heat that must be absorbed by 10.0 g of ice at -20°C to convert it to liquid water at 60.0°C.Given: specific heat (ice)= 2.1 J/g·°C; specific heat (water)= 4.18 J/g·°C; $\Delta$Hfus = 6.0 kJ/mol.

Accepted Answer

A) 63 kJ 
B) 7.5 J 
C) 420 J 
D) 2,900 J 
E) 6,300 J

Question 14

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

Accepted Answer

A) PH3 
B) H2 
C) H2S 
D) CH4 
E) NH3

Question 15

How much energy (heat)is required to convert 52.0 g of ice at -10.0°C to steam at 100°C?

Accepted Answer

A) 40.2 kJ 
B) 157.8 kJ 
C) 1,086 kJ 
D) 2,570 kJ 
E) 22,957 kJ

Question 16

Indicate all the types of intermolecular forces of attraction in HCl(g).

Accepted Answer

The answer of Indicate all the types of intermolecular forces...

Question 17

Which one of the following substances crystallizes as a covalent crystal?

Accepted Answer

A) CaO 
B) SiO2 
C) CO2 
D) Pb 
E) KMnO4

Question 18

Which of the following is not true with regard to water?

Accepted Answer

A) Water has a high heat capacity. 
B) Water has an unusually high boiling point. 
C) Water can form hydrogen bonds. 
D) Ice is more dense than liquid water. 
E) Water is a polar molecule.

Question 19

Given the following liquids and their boiling points, which has the highest vapor pressure at its normal boiling point?

Accepted Answer

A) ethanol, bp = 78°C 
B) methanol, bp = 65°C 
C) water, bp = 100°C 
D) benzene, bp = 80°C 
E) The vapor pressure of each of the liquids at its normal boiling point would be the same.

Question 20

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°C to H2O(l)at 85.0°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

Exam 11: Intermolecular Forces and Liquids and Solids

Arrange the following substances in order of increasing boiling point: CH₃CH₂OH, HOCH₂CH₂OH, CH₃CH₂Cl, and ClCH₂CH₂OH

Identify the dominant (strongest)type of intermolecular force present in Cl₂(l).

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

The specific heat of liquid ethanol, C₂H₅OH(l) , is 2.46 J/g·°C and the heat of vaporization is 39.3 kJ/mol.The boiling point of ethanol is 78.3 °C.What amount of enthalpy is required to heat 50.0 g of liquid ethanol from 23.0 °C to ethanol vapor at 78.3 °C?

Potassium crystallizes in a body-centered cubic lattice.How many atoms are there per unit cell?

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?

Indicate all the types of intermolecular forces of attraction in He(l).

Sodium iodide, NaI, melts at 651°C.In its liquid state NaI conducts electricity.What kind of crystal is this?

What mass of water would need to evaporate from your skin in order to dissipate 1.7 × 10⁵ J of heat from your body? H₂O(l) $\rarr$ H₂O(g) $\Delta$ H_vap = 40.7 kJ/mol

Identify the dominant (strongest)type of intermolecular force present in H₂S(g).

An example of a covalent network solid is

Which of the following phase changes is exothermic?

Calculate the amount of heat that must be absorbed by 10.0 g of ice at -20°C to convert it to liquid water at 60.0°C.Given: specific heat (ice) = 2.1 J/g·°C; specific heat (water) = 4.18 J/g·°C; $\Delta$ H_fus = 6.0 kJ/mol.

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

How much energy (heat) is required to convert 52.0 g of ice at -10.0°C to steam at 100°C?

Indicate all the types of intermolecular forces of attraction in HCl(g).

Which one of the following substances crystallizes as a covalent crystal?

Which of the following is not true with regard to water?

Given the following liquids and their boiling points, which has the highest vapor pressure at its normal boiling point?

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°C to H₂O(l) at 85.0°C? I. $\Delta$ H_fus (H₂O) II. $\Delta$ H_vap (H₂O) III.specific heat of H₂O(s) IV.specific heat of H₂O(l) V.specific heat of H₂O(g)

Exam 11: Intermolecular Forces and Liquids and Solids

Arrange the following substances in order of increasing boiling point: CH3CH2OH, HOCH2CH2OH, CH3CH2Cl, and ClCH2CH2OH

Identify the dominant (strongest)type of intermolecular force present in Cl2(l).

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

The specific heat of liquid ethanol, C2H5OH(l) , is 2.46 J/g·°C and the heat of vaporization is 39.3 kJ/mol.The boiling point of ethanol is 78.3 °C.What amount of enthalpy is required to heat 50.0 g of liquid ethanol from 23.0 °C to ethanol vapor at 78.3 °C?

Potassium crystallizes in a body-centered cubic lattice.How many atoms are there per unit cell?

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?

Indicate all the types of intermolecular forces of attraction in He(l).

Sodium iodide, NaI, melts at 651°C.In its liquid state NaI conducts electricity.What kind of crystal is this?

What mass of water would need to evaporate from your skin in order to dissipate 1.7 × 105 J of heat from your body? H2O(l) →\rarr→ H2O(g) Δ\DeltaΔ Hvap = 40.7 kJ/mol

Identify the dominant (strongest)type of intermolecular force present in H2S(g).

An example of a covalent network solid is

Which of the following phase changes is exothermic?

Calculate the amount of heat that must be absorbed by 10.0 g of ice at -20°C to convert it to liquid water at 60.0°C.Given: specific heat (ice) = 2.1 J/g·°C; specific heat (water) = 4.18 J/g·°C; Δ\DeltaΔ Hfus = 6.0 kJ/mol.

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

How much energy (heat) is required to convert 52.0 g of ice at -10.0°C to steam at 100°C?

Indicate all the types of intermolecular forces of attraction in HCl(g).

Which one of the following substances crystallizes as a covalent crystal?

Which of the following is not true with regard to water?

Given the following liquids and their boiling points, which has the highest vapor pressure at its normal boiling point?

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°C to H2O(l) at 85.0°C? I. Δ\DeltaΔ Hfus (H2O) II. Δ\DeltaΔ Hvap (H2O) III.specific heat of H2O(s) IV.specific heat of H2O(l) V.specific heat of H2O(g)

Arrange the following substances in order of increasing boiling point: CH₃CH₂OH, HOCH₂CH₂OH, CH₃CH₂Cl, and ClCH₂CH₂OH

Identify the dominant (strongest)type of intermolecular force present in Cl₂(l).

The specific heat of liquid ethanol, C₂H₅OH(l) , is 2.46 J/g·°C and the heat of vaporization is 39.3 kJ/mol.The boiling point of ethanol is 78.3 °C.What amount of enthalpy is required to heat 50.0 g of liquid ethanol from 23.0 °C to ethanol vapor at 78.3 °C?

What mass of water would need to evaporate from your skin in order to dissipate 1.7 × 10⁵ J of heat from your body? H₂O(l) $\rarr$ H₂O(g) $\Delta$ H_vap = 40.7 kJ/mol

Identify the dominant (strongest)type of intermolecular force present in H₂S(g).

Calculate the amount of heat that must be absorbed by 10.0 g of ice at -20°C to convert it to liquid water at 60.0°C.Given: specific heat (ice) = 2.1 J/g·°C; specific heat (water) = 4.18 J/g·°C; $\Delta$ H_fus = 6.0 kJ/mol.

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°C to H₂O(l) at 85.0°C? I. $\Delta$ H_fus (H₂O) II. $\Delta$ H_vap (H₂O) III.specific heat of H₂O(s) IV.specific heat of H₂O(l) V.specific heat of H₂O(g)