Question 1

What is the gas found within a bubble of boiling water?

Accepted Answer

A)  air 
B)  chlorine from the water 
C)  water vapor 
D)  hydrogen 
A)  air 
B)  chlorine from the water 
C)  water vapor 
D)  hydrogen

Question 2

Antarctica, which is mostly ice, is much colder than the Arctic, which is a mixture of ice and water. Why?

Accepted Answer

A)  The liquid water of the Arctic Ocean absorbs and releases a lot of heat that keeps the temperatures in that region from fluctuating. 
B)  The Arctic is much farther north than the Antarctic. 
C)  The salt in the water of the Antarctic keeps the water from freezing. 
D)  The specific heat of the ice is less than that of liquid water, which allows its temperature to change more readily. 
E)  Two of the above are reasonable. 
A)  The liquid water of the Arctic Ocean absorbs and releases a lot of heat that keeps the temperatures in that region from fluctuating. 
B)  The Arctic is much farther north than the Antarctic. 
C)  The salt in the water of the Antarctic keeps the water from freezing. 
D)  The specific heat of the ice is less than that of liquid water, which allows its temperature to change more readily. 
E)  Two of the above are reasonable.

Question 3

Which of the following weather effects would not be attributed to water's high specific heat?

Accepted Answer

A)  The winter in San Francisco is milder than the winter in Washington, D.C. 
B)  The weather in Stockholm, Sweden (which is at the same latitude as Fairbanks, Alaska), is very mild. 
C)  The temperature in the Mojave desert fluctuates wildly, being very hot during the day and very cold at night. 
D)  Europe is much warmer than Canada. 
E)  All of the above are due to water. 
A)  The winter in San Francisco is milder than the winter in Washington, D.C. 
B)  The weather in Stockholm, Sweden (which is at the same latitude as Fairbanks, Alaska), is very mild. 
C)  The temperature in the Mojave desert fluctuates wildly, being very hot during the day and very cold at night. 
D)  Europe is much warmer than Canada. 
E)  All of the above are due to water.

Question 4

Why does evaporation cool a liquid?

Accepted Answer

A)  The departing gas molecule takes some kinetic energy with it as it leaves the surface. 
B)  The overall heat decreases because the air cools. 
C)  The average energy of the system increases because of the increased disorder in the new gas molecules. 
D)  The gas molecules need to transfer their kinetic energy to the new slower gas molecule. 
E)  none of the above 
A)  The departing gas molecule takes some kinetic energy with it as it leaves the surface. 
B)  The overall heat decreases because the air cools. 
C)  The average energy of the system increases because of the increased disorder in the new gas molecules. 
D)  The gas molecules need to transfer their kinetic energy to the new slower gas molecule. 
E)  none of the above

Question 5

Given the following specific heats and that each sample had the same mass, which would require the greatest amount of heat energy to increase its temperature 50°C?

Accepted Answer

A)  ammonia, 4.70 J/(g°
C)  
B)  water, 4.184 J/(g°
C)  
C)  aluminum, 0.90 J/(g°
C)  
D)  silver, 0.24 J/(g°
C)  
E)  All of the above require the same amount of heat energy. 
A)  ammonia, 4.70 J/(g°
C)  
B)  water, 4.184 J/(g°
C)  
C)  aluminum, 0.90 J/(g°
C)  
D)  silver, 0.24 J/(g°
C)  
E)  All of the above require the same amount of heat energy.

Question 6

What happens to the freezing temperature of a salt water solution as it becomes more concentrated?

Accepted Answer

A)  As salt water becomes more concentrated, the temperature at which it freezes become lower because fewer water molecules of the liquid phase in contact with the ice. 
B)  As salt water becomes more concentrated, the temperature at which it freezes become higher because salt ions help to hold together the ice. 
C)  As salt water becomes more concentrated, the temperature at which it freezes does not change. 
D)  As salt water becomes more concentrated, the temperature at which it freezes become higher because the molecules are moving faster as they interact with the salt ions. 
A)  As salt water becomes more concentrated, the temperature at which it freezes become lower because fewer water molecules of the liquid phase in contact with the ice. 
B)  As salt water becomes more concentrated, the temperature at which it freezes become higher because salt ions help to hold together the ice. 
C)  As salt water becomes more concentrated, the temperature at which it freezes does not change. 
D)  As salt water becomes more concentrated, the temperature at which it freezes become higher because the molecules are moving faster as they interact with the salt ions.

Question 7

Relative to pure water, an aqueous sugar solution ________.

Accepted Answer

A)  has a lower freezing point because crystal formation is inhibited by the sugar molecules 
B)  has the same freezing point because most of the solution is water molecules 
C)  has a higher freezing point because crystal formation is promoted by the sugar molecules 
D)  has a lower freezing point because crystal formation is promoted by the sugar molecules 
E)  has a higher freezing point because crystal formation is inhibited by the sugar molecules 
A)  has a lower freezing point because crystal formation is inhibited by the sugar molecules 
B)  has the same freezing point because most of the solution is water molecules 
C)  has a higher freezing point because crystal formation is promoted by the sugar molecules 
D)  has a lower freezing point because crystal formation is promoted by the sugar molecules 
E)  has a higher freezing point because crystal formation is inhibited by the sugar molecules

Question 8

Water will boil spontaneously in a vacuum. Could you cook an egg in this boiling water?

Accepted Answer

A)  Yes, since the water is boiling it has enough energy to cook the egg even if it is at room temperature. 
B)  No, because food is cooked by the transfer of thermal energy from the water to the food, and water at room temperature does not have enough thermal energy to cook an egg. 
C)  Yes, since the food is not under pressure in the vacuum, it will also cook at a much lower temperature. 
D)  No, the food would not cook because the thermal energy could not be transferred to the food in a vacuum. 
A)  Yes, since the water is boiling it has enough energy to cook the egg even if it is at room temperature. 
B)  No, because food is cooked by the transfer of thermal energy from the water to the food, and water at room temperature does not have enough thermal energy to cook an egg. 
C)  Yes, since the food is not under pressure in the vacuum, it will also cook at a much lower temperature. 
D)  No, the food would not cook because the thermal energy could not be transferred to the food in a vacuum.

Question 9

Which of the following describes what happens when you increase the temperature of water?

Accepted Answer

A)  The molecules start to vibrate and move farther apart. 
B)  The molecules start to vibrate and move closer together. 
C)  The molecular vibrations start to slow and the molecules move farther apart. 
D)  The molecular vibrations start to slow and the molecules move closer together. 
E)  none of the above. 
A)  The molecules start to vibrate and move farther apart. 
B)  The molecules start to vibrate and move closer together. 
C)  The molecular vibrations start to slow and the molecules move farther apart. 
D)  The molecular vibrations start to slow and the molecules move closer together. 
E)  none of the above.

Question 10

If the specific heat of aluminum is 0.90 J/(g°C), how much heat is needed to raise the temperature of a 10.0-gram piece by 20.0°C?

Accepted Answer

A)  180 J 
B)  222 J 
C)  200 J 
D)  90 J 
E)  0.9 J 
A)  180 J 
B)  222 J 
C)  200 J 
D)  90 J 
E)  0.9 J

Question 11

From the diagram above describing the phase of water relative to temperature and pressure, at which point does water exist in all three phases?

Accepted Answer

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

Question 12

Describe how a boiling liquid can be used to cool something (i.e., a refrigerator).

Accepted Answer

A)  A low boiling liquid absorbs heat energy, dropping the temperature. 
B)  As a liquid condenses, heat energy is required and the temperature drops. 
C)  Heat energy is only used with solids like ice. 
D)  Heat is used to convert vapor into a liquid, which is cooler than a gas. 
E)  none of the above 
A)  A low boiling liquid absorbs heat energy, dropping the temperature. 
B)  As a liquid condenses, heat energy is required and the temperature drops. 
C)  Heat energy is only used with solids like ice. 
D)  Heat is used to convert vapor into a liquid, which is cooler than a gas. 
E)  none of the above

Question 13

Capillary action causes water to climb up the internal walls of narrow glass tubes. Why does the water not climb so high when the glass tube is wider?

Accepted Answer

A)  The upper surface area is exposed to greater atmospheric pressure. 
B)  A wider column of water weighs more. 
C)  The water sticks better to the glass because of the greater surface area of contact. 
D)  The greater rate of evaporation has the effect of pushing the water back downwards. 
A)  The upper surface area is exposed to greater atmospheric pressure. 
B)  A wider column of water weighs more. 
C)  The water sticks better to the glass because of the greater surface area of contact. 
D)  The greater rate of evaporation has the effect of pushing the water back downwards.

Question 14

What is the temperature change if you heat water from 55°C to 100°C?

Accepted Answer

A)  55°C 
B)  100°C 
C)  45°C 
D)  -45°C 
E)  -55°C 
A)  55°C 
B)  100°C 
C)  45°C 
D)  -45°C 
E)  -55°C

Question 15

What is found within the extra volume that arises as water expands upon freezing?

Accepted Answer

A)  nothing 
B)  other water molecules 
C)  air 
D)  dissolved oxygen 
E)  the atoms have expanded 
A)  nothing 
B)  other water molecules 
C)  air 
D)  dissolved oxygen 
E)  the atoms have expanded

Question 16

If you were somehow able to sit at the surface of an ice cube and were able to slow the movement of water molecules from the solid to the liquid phase, what would eventually happen to the ice cube?

Accepted Answer

A)  It would increase in size. 
B)  It would melt because you are sitting on it and you give off heat. 
C)  It would melt because you have slowed the rate of water uptake. 
D)  It would melt because you have increased the rate of water uptake. 
E)  none of the above 
A)  It would increase in size. 
B)  It would melt because you are sitting on it and you give off heat. 
C)  It would melt because you have slowed the rate of water uptake. 
D)  It would melt because you have increased the rate of water uptake. 
E)  none of the above

Question 17

For an ice/water mixture at 0°C, which is true?

Accepted Answer

A)  The rate at which ice melts is faster. 
B)  The rate at which water freezes is faster 
C)  The rate at which ice melts and freezes are both equal. 
D)  Ice always freezes at 0°C. 
E)  Ice always melts at 0°C. 
A)  The rate at which ice melts is faster. 
B)  The rate at which water freezes is faster 
C)  The rate at which ice melts and freezes are both equal. 
D)  Ice always freezes at 0°C. 
E)  Ice always melts at 0°C.

Question 18

Which of the following statements does not describe a property of water?

Accepted Answer

A)  You are made mostly of water. 
B)  It is the only molecule that is found in all three phases (solid, liquid, gas) in large quantities on the planet. 
C)  Water is very resistant to a change in temperature. 
D)  Many of the properties of water are a direct consequence of the intermolecular attractions between water molecules. 
E)  The hydrogens of a water molecule have a partial negative charge. 
A)  You are made mostly of water. 
B)  It is the only molecule that is found in all three phases (solid, liquid, gas) in large quantities on the planet. 
C)  Water is very resistant to a change in temperature. 
D)  Many of the properties of water are a direct consequence of the intermolecular attractions between water molecules. 
E)  The hydrogens of a water molecule have a partial negative charge.

Question 19

As an ice cube floating in a glass of water melts, what happens to the water level?

Accepted Answer

A)  The water level rises to the point where the ice floats above the water. 
B)  As the ice melts, the water level does not change-the melting ice "caves in" and exactly fills the open spaces. 
C)  The melting ice "caves in" and fills the open spaces-therefore the water level is lower after the ice melts. 
A)  The water level rises to the point where the ice floats above the water. 
B)  As the ice melts, the water level does not change-the melting ice "caves in" and exactly fills the open spaces. 
C)  The melting ice "caves in" and fills the open spaces-therefore the water level is lower after the ice melts.

Question 20

What normally describes what happens when you decrease the temperature of water?

Accepted Answer

A)  The molecules start to vibrate and move farther apart, increasing the density. 
B)  The molecules start to vibrate and move closer together, increasing the density. 
C)  The molecular vibrations start to slow and the molecules move farther apart, decreasing the density. 
D)  The molecular vibrations start to slow and the molecules move closer together, increasing the density. 
E)  none of the above 
A)  The molecules start to vibrate and move farther apart, increasing the density. 
B)  The molecules start to vibrate and move closer together, increasing the density. 
C)  The molecular vibrations start to slow and the molecules move farther apart, decreasing the density. 
D)  The molecular vibrations start to slow and the molecules move closer together, increasing the density. 
E)  none of the above

What is the gas found within a bubble of boiling water?

Antarctica, which is mostly ice, is much colder than the Arctic, which is a mixture of ice and water. Why?

Which of the following weather effects would not be attributed to water's high specific heat?

Why does evaporation cool a liquid?

Given the following specific heats and that each sample had the same mass, which would require the greatest amount of heat energy to increase its temperature 50°C?

What happens to the freezing temperature of a salt water solution as it becomes more concentrated?

Relative to pure water, an aqueous sugar solution ________.

Water will boil spontaneously in a vacuum. Could you cook an egg in this boiling water?

Which of the following describes what happens when you increase the temperature of water?

If the specific heat of aluminum is 0.90 J/(g°C), how much heat is needed to raise the temperature of a 10.0-gram piece by 20.0°C?

From the diagram above describing the phase of water relative to temperature and pressure, at which point does water exist in all three phases?

Describe how a boiling liquid can be used to cool something (i.e., a refrigerator).

Capillary action causes water to climb up the internal walls of narrow glass tubes. Why does the water not climb so high when the glass tube is wider?

What is the temperature change if you heat water from 55°C to 100°C?

What is found within the extra volume that arises as water expands upon freezing?

If you were somehow able to sit at the surface of an ice cube and were able to slow the movement of water molecules from the solid to the liquid phase, what would eventually happen to the ice cube?

For an ice/water mixture at 0°C, which is true?

Which of the following statements does not describe a property of water?

As an ice cube floating in a glass of water melts, what happens to the water level?

What normally describes what happens when you decrease the temperature of water?

About Science

Particles of Matter

Elements of Chemistry

Subatomic Particles

The Atomic Nucleus

How Atoms Bond

How Molecules Mix

How Chemicals React

Acids and Bases in Our Environment

Oxidations and Reductions Charge the World

Organic Compounds

Nutrients of Life

Medicinal Chemistry

Optimizing Food Production

Protection Water and Air Resources

Capturing Energy

Filters

Exam 8: How Water Behaves

What is the gas found within a bubble of boiling water?

Antarctica, which is mostly ice, is much colder than the Arctic, which is a mixture of ice and water. Why?

Which of the following weather effects would not be attributed to water's high specific heat?

Why does evaporation cool a liquid?

Given the following specific heats and that each sample had the same mass, which would require the greatest amount of heat energy to increase its temperature 50°C?

What happens to the freezing temperature of a salt water solution as it becomes more concentrated?

Relative to pure water, an aqueous sugar solution ________.

Water will boil spontaneously in a vacuum. Could you cook an egg in this boiling water?

Which of the following describes what happens when you increase the temperature of water?

If the specific heat of aluminum is 0.90 J/(g°C), how much heat is needed to raise the temperature of a 10.0-gram piece by 20.0°C?

From the diagram above describing the phase of water relative to temperature and pressure, at which point does water exist in all three phases?

Describe how a boiling liquid can be used to cool something (i.e., a refrigerator).

Capillary action causes water to climb up the internal walls of narrow glass tubes. Why does the water not climb so high when the glass tube is wider?

What is the temperature change if you heat water from 55°C to 100°C?

What is found within the extra volume that arises as water expands upon freezing?

If you were somehow able to sit at the surface of an ice cube and were able to slow the movement of water molecules from the solid to the liquid phase, what would eventually happen to the ice cube?

For an ice/water mixture at 0°C, which is true?

Which of the following statements does not describe a property of water?

As an ice cube floating in a glass of water melts, what happens to the water level?

What normally describes what happens when you decrease the temperature of water?

About Science

Particles of Matter

Elements of Chemistry

Subatomic Particles

The Atomic Nucleus

How Atoms Bond

How Molecules Mix

How Chemicals React

Acids and Bases in Our Environment

Oxidations and Reductions Charge the World

Organic Compounds

Nutrients of Life

Medicinal Chemistry

Optimizing Food Production

Protection Water and Air Resources

Capturing Energy

Filters