Question 1

A material with a high specific heat ________.

Accepted Answer

A)  takes a lot of energy to change its temperature 
B)  melts at a high temperature 
C)  rapidly cools, giving up its heat 
D)  changes temperature very rapidly when heated 
E)  takes a very small temperature change to change the amount of heat in a material 
A)  takes a lot of energy to change its temperature 
B)  melts at a high temperature 
C)  rapidly cools, giving up its heat 
D)  changes temperature very rapidly when heated 
E)  takes a very small temperature change to change the amount of heat in a material

Question 2

Why does transforming water from 100°C liquid to 100°C gas require much more energy than to raise the temperature of the same amount of water from absolute zero all the way to 100°C liquid?

Accepted Answer

A)  While water is in the solid phase, it is only necessary to impart energy to the water molecules themselves. Once in the liquid phase much more heat is required to impart sufficient energy to the molecules because there is more volume present. 
B)  False! It does not require more energy to transform water from 100°C liquid to 100°C gas than to raise the temperature of the same amount of water from absolute zero all the way to 100°C liquid. 
C)  Transforming water from 100°C liquid to 100°C gas requires breaking the hydrogen bonds between the liquid molecules. 
D)  The amount of heat required to raise the temperature of the water or transform its phase is directly proportional to the densities of the water molecules involved. Obviously, driving liquid water to the vapor will drastically change its density. 
A)  While water is in the solid phase, it is only necessary to impart energy to the water molecules themselves. Once in the liquid phase much more heat is required to impart sufficient energy to the molecules because there is more volume present. 
B)  False! It does not require more energy to transform water from 100°C liquid to 100°C gas than to raise the temperature of the same amount of water from absolute zero all the way to 100°C liquid. 
C)  Transforming water from 100°C liquid to 100°C gas requires breaking the hydrogen bonds between the liquid molecules. 
D)  The amount of heat required to raise the temperature of the water or transform its phase is directly proportional to the densities of the water molecules involved. Obviously, driving liquid water to the vapor will drastically change its density.

Question 3

Would fevers run higher or lower if water's specific heat were not so high?

Accepted Answer

A)  With a lower specific heat, water would require a higher energy input to change its temperature. Our fevers, therefore, would run at a lower temperature. 
B)  With a lower specific heat, water would gain a higher temperature for the same amount of energy input. Our fevers, therefore, would run at a higher temperature. 
C)  A lower specific heat would not effect its ability to change waters temperature, so it would not have an effect on our fevers. 
D)  With a lower specific heat, our bodies would evaporate (sweat) twice as much water, therefore our fevers would be lower. 
A)  With a lower specific heat, water would require a higher energy input to change its temperature. Our fevers, therefore, would run at a lower temperature. 
B)  With a lower specific heat, water would gain a higher temperature for the same amount of energy input. Our fevers, therefore, would run at a higher temperature. 
C)  A lower specific heat would not effect its ability to change waters temperature, so it would not have an effect on our fevers. 
D)  With a lower specific heat, our bodies would evaporate (sweat) twice as much water, therefore our fevers would be lower.

Question 4

Boiling is when the ________.

Accepted Answer

A)  vapor pressure of a liquid equals the atmospheric pressure 
B)  rate of evaporation equals the rate of condensation 
C)  material no longer undergoes condensation 
D)  vapor pressure decreases to zero 
E)  none of the above 
A)  vapor pressure of a liquid equals the atmospheric pressure 
B)  rate of evaporation equals the rate of condensation 
C)  material no longer undergoes condensation 
D)  vapor pressure decreases to zero 
E)  none of the above

Question 5

Why do ice skates work?

Accepted Answer

A)  The pressure of the blades on the ice creates a temporary water layer. 
B)  The pressure of the blades cuts a hole in the ice and water flows in. 
C)  The blades are treated with a chemical that melts the ice temporarily, which creates a water layer. 
D)  Ice is naturally slippery. 
A)  The pressure of the blades on the ice creates a temporary water layer. 
B)  The pressure of the blades cuts a hole in the ice and water flows in. 
C)  The blades are treated with a chemical that melts the ice temporarily, which creates a water layer. 
D)  Ice is naturally slippery.

Question 6

Water has a low specific heat because of its ________.

Accepted Answer

A)  transparency 
B)  density 
C)  polarity 
D)  phase 
E)  Water actually has a high specific heat. 
A)  transparency 
B)  density 
C)  polarity 
D)  phase 
E)  Water actually has a high specific heat.

Question 7

What happens to two water molecules after they come together to form a hydrogen bond-do they vibrate more rapidly or less rapidly?

Accepted Answer

A)  Since the bonding of the two water molecules results in a loss of kinetic energy, the molecules would vibrate less rapidly. 
B)  Since the bonding of the two water molecules results in an increase of kinetic energy, the molecules would vibrate more rapidly. 
C)  Since the bonding of the two water molecules results in no change in kinetic energy, the vibration of the molecules does not change. 
D)  The formation of the hydrogen bond stabilizes both molecules. The vibration rate is therefore less rapid. 
A)  Since the bonding of the two water molecules results in a loss of kinetic energy, the molecules would vibrate less rapidly. 
B)  Since the bonding of the two water molecules results in an increase of kinetic energy, the molecules would vibrate more rapidly. 
C)  Since the bonding of the two water molecules results in no change in kinetic energy, the vibration of the molecules does not change. 
D)  The formation of the hydrogen bond stabilizes both molecules. The vibration rate is therefore less rapid.

Question 8

Should the specific heat of your automobile's radiator fluid be as high as possible or as low as possible? Why?

Accepted Answer

A)  A higher specific heat radiator fluid would be more effective at distributing the heat to different parts of the engine so it doesn't all build up in one place. 
B)  A lower specific heat would mean that it is starting at a low temperature, and has to heat up to a much higher temperature before it boils away. 
C)  A higher specific heat radiator fluid would be more effective at absorbing heat from the engine, so that it doesn't melt. 
D)  A lower specific heat radiator fluid means that its molecules will not form a thick solution, but rather will get "thinner" as it is heated so that it won't block up the radiator. 
A)  A higher specific heat radiator fluid would be more effective at distributing the heat to different parts of the engine so it doesn't all build up in one place. 
B)  A lower specific heat would mean that it is starting at a low temperature, and has to heat up to a much higher temperature before it boils away. 
C)  A higher specific heat radiator fluid would be more effective at absorbing heat from the engine, so that it doesn't melt. 
D)  A lower specific heat radiator fluid means that its molecules will not form a thick solution, but rather will get "thinner" as it is heated so that it won't block up the radiator.

Question 9

Your instructor hands you a closed flask of room-temperature water. When you hold it, the heat from your bare hands causes the water to boil. Quite impressive! How is this accomplished?

Accepted Answer

A)  The pressure inside the flask is very high, so only a slight increase in temperature is required to bring the water to a boil. 
B)  Your instructor has tricked you and there must be a liquid, such as alcohol, with a lower boiling point than water. 
C)  A salt must be dissolved in the water to lower its boiling point. 
D)  The air in the flask is very low in pressure, so that the heat from your hand (not the pressure from your hand) will produce boiling at this reduced pressure. 
A)  The pressure inside the flask is very high, so only a slight increase in temperature is required to bring the water to a boil. 
B)  Your instructor has tricked you and there must be a liquid, such as alcohol, with a lower boiling point than water. 
C)  A salt must be dissolved in the water to lower its boiling point. 
D)  The air in the flask is very low in pressure, so that the heat from your hand (not the pressure from your hand) will produce boiling at this reduced pressure.

Question 10

It is important to protect water pipes in your home from freezing because ________.

Accepted Answer

A)  freezing water will scrape the lining from the insides of the pipes 
B)  water expands more than the pipe material, which will fracture the pipes if water in them freezes 
C)  blocked water behind the frozen ice will build up pressure and will burst the pipes 
D)  the ice will promote serious erosion of the pipe material 
E)  all of the above 
A)  freezing water will scrape the lining from the insides of the pipes 
B)  water expands more than the pipe material, which will fracture the pipes if water in them freezes 
C)  blocked water behind the frozen ice will build up pressure and will burst the pipes 
D)  the ice will promote serious erosion of the pipe material 
E)  all of the above

Question 11

If all of the liquids pictured above were the same, which setup would contain the capillary with the smallest diameter?

Accepted Answer

A)  a 
B)  b 
C)  c 
D)  d 
E)  e 
A)  a 
B)  b 
C)  c 
D)  d 
E)  e

Question 12

Does putting a lid over a pot of water on a stove shorten the time it takes for the water to come to a boil? After the water is boiling, does use of the lid shorten the cooking time of food?

Accepted Answer

A)  No, the boiling point of water is always 100°C, so the lid would have no effect on how long it takes for water to reach that temperature. however, food cooks faster with a lid because heat is held inside the pot. 
B)  Yes, since the pressure is increased under the lid the boiling temperature is lower; however, after the water boils, the increased pressure would prevent gas bubbles from escaping so the food cooks in about the same amount of time as without a lid. 
C)  Yes, the trapped heat quickens boiling; the lid also increases pressure on the boiling water which raises its boiling temperature, cooking food in a shorter time. 
D)  No, it takes longer to boil the water because the increased pressure in the pot raises water's boiling point. Food will cook faster because the temperature of the water is higher. 
A)  No, the boiling point of water is always 100°C, so the lid would have no effect on how long it takes for water to reach that temperature. however, food cooks faster with a lid because heat is held inside the pot. 
B)  Yes, since the pressure is increased under the lid the boiling temperature is lower; however, after the water boils, the increased pressure would prevent gas bubbles from escaping so the food cooks in about the same amount of time as without a lid. 
C)  Yes, the trapped heat quickens boiling; the lid also increases pressure on the boiling water which raises its boiling temperature, cooking food in a shorter time. 
D)  No, it takes longer to boil the water because the increased pressure in the pot raises water's boiling point. Food will cook faster because the temperature of the water is higher.

Question 13

Ice is slippery because ________.

Accepted Answer

A)  air molecules have been excluded 
B)  of greater kinetic energy at the surface 
C)  of its relatively high purity 
D)  surface crystals fall apart 
E)  of its tight internal and external structuring 
A)  air molecules have been excluded 
B)  of greater kinetic energy at the surface 
C)  of its relatively high purity 
D)  surface crystals fall apart 
E)  of its tight internal and external structuring

Question 14

A water bug can rest on top of water without getting wet because of ________.

Accepted Answer

A)  surface tension 
B)  cohesive forces within water 
C)  its nonpolar exterior 
D)  all of the above 
A)  surface tension 
B)  cohesive forces within water 
C)  its nonpolar exterior 
D)  all of the above

Question 15

Which statement best describes what is happening at the surface of liquid water?

Accepted Answer

A)  At the surface there is a constant exchange of liquid and gaseous water. 
B)  Fast moving water molecules leave the surface and become gas molecules. 
C)  Slow moving gas molecules are captured by the liquid water. 
D)  The gas molecules exchange with the liquid molecules. 
E)  all of the above 
A)  At the surface there is a constant exchange of liquid and gaseous water. 
B)  Fast moving water molecules leave the surface and become gas molecules. 
C)  Slow moving gas molecules are captured by the liquid water. 
D)  The gas molecules exchange with the liquid molecules. 
E)  all of the above

Question 16

What is the leading cause of surface tension in water?

Accepted Answer

A)  hydrogen bonding 
B)  ion-dipole interactions 
C)  solvation 
D)  evaporation 
A)  hydrogen bonding 
B)  ion-dipole interactions 
C)  solvation 
D)  evaporation

Question 17

Would you expect the surface tension of water to increase or decrease with temperature?

Accepted Answer

A)  At warmer temperatures water molecules are moving faster. This increased friction produces a stronger electrical charge, causing them to cohere more strongly, which increases surface tension. 
B)  At cooler temperatures water molecules are moving slower, which makes it relatively easy for them to cohere to one another. This, in turn, increases the surface tension. 
C)  At warmer temperatures water molecules are moving faster, which makes it easier for them to bump into and cohere to one another, which increases surface tension. 
D)  At cooler temperatures, the water molecules adhere more strongly to each other because they condense as the reach freezing point, which increases surface tension. 
A)  At warmer temperatures water molecules are moving faster. This increased friction produces a stronger electrical charge, causing them to cohere more strongly, which increases surface tension. 
B)  At cooler temperatures water molecules are moving slower, which makes it relatively easy for them to cohere to one another. This, in turn, increases the surface tension. 
C)  At warmer temperatures water molecules are moving faster, which makes it easier for them to bump into and cohere to one another, which increases surface tension. 
D)  At cooler temperatures, the water molecules adhere more strongly to each other because they condense as the reach freezing point, which increases surface tension.

Question 18

If water had a lower specific heat, would ponds be more likely to freeze or less likely to freeze?

Accepted Answer

A)  Ponds would take less time to freeze because they couldn't hold on to heat so well. 
B)  Water would necessarily also have a lower freezing point, and it would take more time for a pond to freeze. 
C)  A pond would take less time to freeze because the water molecules would slow down at a slower rate. 
D)  Ponds would take more time to freeze because ice would no longer be less dense than liquid water. 
A)  Ponds would take less time to freeze because they couldn't hold on to heat so well. 
B)  Water would necessarily also have a lower freezing point, and it would take more time for a pond to freeze. 
C)  A pond would take less time to freeze because the water molecules would slow down at a slower rate. 
D)  Ponds would take more time to freeze because ice would no longer be less dense than liquid water.

Question 19

Why does water not freeze at 0°C when either ions or molecules other than   O are present?

Accepted Answer

A)  Molecules or ions dissolved in the water give the water molecules something else to easily bond with, thus allowing the solution to freeze well above 0°C. 
B)  Molecules or ions dissolved in the water increase the number of water molecules at the solid-liquid interface, thus allowing for the rate of ice formation to increase at a temperature above 0°C. 
C)  When molecules or ions are dissolved in the water, these solute molecules both take up space and inhibit the formation of the solid phase, thus lowering the freezing point temperature below 0°C. 
D)  Molecules or ions dissolved in the water will sometimes raise the freezing point above 0°C and other times lower it below 0°C depending on the nature of these solute particles. 
A)  Molecules or ions dissolved in the water give the water molecules something else to easily bond with, thus allowing the solution to freeze well above 0°C. 
B)  Molecules or ions dissolved in the water increase the number of water molecules at the solid-liquid interface, thus allowing for the rate of ice formation to increase at a temperature above 0°C. 
C)  When molecules or ions are dissolved in the water, these solute molecules both take up space and inhibit the formation of the solid phase, thus lowering the freezing point temperature below 0°C. 
D)  Molecules or ions dissolved in the water will sometimes raise the freezing point above 0°C and other times lower it below 0°C depending on the nature of these solute particles.

Question 20

Why does evaporation of a liquid also cool the gas above it?

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

A material with a high specific heat ________.

Why does transforming water from 100°C liquid to 100°C gas require much more energy than to raise the temperature of the same amount of water from absolute zero all the way to 100°C liquid?

Would fevers run higher or lower if water's specific heat were not so high?

Boiling is when the ________.

Why do ice skates work?

Water has a low specific heat because of its ________.

What happens to two water molecules after they come together to form a hydrogen bond-do they vibrate more rapidly or less rapidly?

Should the specific heat of your automobile's radiator fluid be as high as possible or as low as possible? Why?

Your instructor hands you a closed flask of room-temperature water. When you hold it, the heat from your bare hands causes the water to boil. Quite impressive! How is this accomplished?

It is important to protect water pipes in your home from freezing because ________.

If all of the liquids pictured above were the same, which setup would contain the capillary with the smallest diameter?

Does putting a lid over a pot of water on a stove shorten the time it takes for the water to come to a boil? After the water is boiling, does use of the lid shorten the cooking time of food?

Ice is slippery because ________.

A water bug can rest on top of water without getting wet because of ________.

Which statement best describes what is happening at the surface of liquid water?

What is the leading cause of surface tension in water?

Would you expect the surface tension of water to increase or decrease with temperature?

If water had a lower specific heat, would ponds be more likely to freeze or less likely to freeze?

Why does water not freeze at 0°C when either ions or molecules other than O are present?

Why does evaporation of a liquid also cool the gas above it?

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

A material with a high specific heat ________.

Why does transforming water from 100°C liquid to 100°C gas require much more energy than to raise the temperature of the same amount of water from absolute zero all the way to 100°C liquid?

Would fevers run higher or lower if water's specific heat were not so high?

Boiling is when the ________.

Why do ice skates work?

Water has a low specific heat because of its ________.

What happens to two water molecules after they come together to form a hydrogen bond-do they vibrate more rapidly or less rapidly?

Should the specific heat of your automobile's radiator fluid be as high as possible or as low as possible? Why?

Your instructor hands you a closed flask of room-temperature water. When you hold it, the heat from your bare hands causes the water to boil. Quite impressive! How is this accomplished?

It is important to protect water pipes in your home from freezing because ________.

If all of the liquids pictured above were the same, which setup would contain the capillary with the smallest diameter?

Does putting a lid over a pot of water on a stove shorten the time it takes for the water to come to a boil? After the water is boiling, does use of the lid shorten the cooking time of food?

Ice is slippery because ________.

A water bug can rest on top of water without getting wet because of ________.

Which statement best describes what is happening at the surface of liquid water?

What is the leading cause of surface tension in water?

Would you expect the surface tension of water to increase or decrease with temperature?

If water had a lower specific heat, would ponds be more likely to freeze or less likely to freeze?

Why does water not freeze at 0°C when either ions or molecules other than O are present?

Why does evaporation of a liquid also cool the gas above it?

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