Question 1

Determine the shift in equilibrium that would result if 100 kJ of energy were removed from a system in which dry ice and CO₂ gas were in equilibrium at the freezing point.

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Question 2

Determine the shift in equilibrium that would result if 100 kJ of energy were added to ice melting at 0°C to form water (H₂O(s)⇆ H₂O(l)).

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Question 3

The vapor pressure of ethanol is 400 mmHg at 63.5°C. Its molar heat of vaporization is 39.3 kJ/mol. What is the vapor pressure of ethanol at 34.9°C?

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Question 4

The molar enthalpy of vaporization of carbon disulfide is 26.74 kJ/mol, and its normal boiling point is 46°C. What is the vapor pressure of CS₂ at 0°C?

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Question 5

Tungsten metal (W)exists as a body-centered cubic structure. How many tungsten atoms are within a unit cell of tungsten metal?

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Question 6

The atomic planes in a graphite crystal are separated by 335 pm. At what angle would you find the second-order (n = 2)diffraction of 0.154 nm X-rays from a graphite crystal?

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Question 7

Describe the difference between molecular crystals and covalent crystals, in terms of types of bonding and physical properties.

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Question 8

Osmium tetroxide, OsO₄, forms a crystal that melts at 40°C. The liquid formed from this melting does not conduct electricity. What would be the best classification of this type of crystal?

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Question 9

An unknown solid is hard, but malleable and melts at 1700°C. The liquid form conducts electricity. The solid form also conducts electricity. What kind of crystal is this?

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Question 10

An unknown solid is hard, but brittle and melts at 3500°C. The liquid form of the unknown conducts electricity, but the solid form does not. What kind of crystal is the unknown?

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Question 11

Above a substance's critical point, its gas phase becomes like a liquid and the liquid becomes like a gas.

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Question 12

When a gas is below its critical temperature, application of sufficient pressure will cause the gas to become a liquid.

Accepted Answer

Below the critical temperature, a gas can be liquefied by applying sufficient pressure, as the molecules are close enough to form a liquid phase.

Question 13

Viscosity is determined only by the intermolecular attractive forces in a liquid.

Accepted Answer

Viscosity is influenced by intermolecular forces, but also by temperature and the size and shape of the molecules.

Question 14

The surface tension of a liquid depends on the strength of the substance's intermolecular attractive forces.

Accepted Answer

Surface tension arises from the cohesive forces between molecules in a liquid, which are determined by the strength of the intermolecular forces.

Question 15

A cylinder contains a liquid which is in equilibrium with its vapor at 45.0^°C. If the piston is moved down to constrict the volume of the cylinder without changing the temperature, the equilibrium vapor pressure of the liquid will increase.

Accepted Answer

The equilibrium vapor pressure of a liquid depends only on the temperature, not on the volume or pressure changes in the container.

Question 16

All substances have London forces.

Accepted Answer

London forces, also known as dispersion forces, are present in all substances because they arise from temporary fluctuations in electron density, which occur in all atoms and molecules.

Question 17

Amorphous solids are highly ordered crystals, and they must contain silicon or carbon to be classified as an amorphous solid.

Accepted Answer

Amorphous solids lack the long-range order characteristic of crystals and do not need to contain silicon or carbon to be classified as such.

Question 18

What is the difference between intermolecular interactions and intramolecular interactions in a molecule?

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Question 19

During a rain storm, the surface of a car hood gets wet. If the car has a good polish or has recently been waxed, the water tends to bead or form drops, instead of evenly covering the surface. What does this say about the properties of water and the wax used to protect the car hood?

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Question 20

Why would the coffee purchased in a to-go cup with a lid at the fast food takeout shop remain hot much longer than the coffee you pour into your ceramic cup at home?

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Quiz 12: Intermolecular Attractions and the Properties of Liquids and Solids

Determine the shift in equilibrium that would result if 100 kJ of energy were removed from a system in which dry ice and CO2 gas were in equilibrium at the freezing point.

Determine the shift in equilibrium that would result if 100 kJ of energy were added to ice melting at 0°C to form water (H2O(s)⇆ H2O(l)).