Preview Extract
Chapter 6 Thermal Energy and Thermodynamics
6.1 Temperature
1) Whether one object is warmer than another object has most to do with
A) molecular kinetic energy.
B) molecular potential energy.
C) heat flow.
D) masses of internal particles.
Answer: A
2) The motion of molecules that most affects temperature is
A) translational motion.
B) rotational motion.
C) oscillatory motion.
D) simple harmonic motion.
Answer: A
3) The temperature of boiling water is
A) 100°C.
B) 212°F.
C) both
Answer: C
4) The temperature of melting ice is
A) 0°C.
B) 32°F.
C) both
Answer: C
5) When you touch a piece of ice with your finger, energy flows
A) from your finger to the ice.
B) from the ice to your finger.
C) both ways
Answer: A
6) When you touch a hot penny in sunlight with your finger, energy flows
A) from your finger to the penny.
B) from the penny to your finger.
C) both ways
Answer: B
7) The motion of particles that contribute to temperature are
A) translational.
B) rotational.
C) circular.
D) orbital.
Answer: A
8) Substances are composed of tiny particles. Temperature is related mostly to the particles'
A) average translational kinetic energy.
B) total kinetic energy.
C) average thermal energy.
D) movement of energy from particle to particle.
E) none of the above
Answer: A
9) The thermal energy in a substance is related mostly to the
A) average translational kinetic energy of particles.
B) total kinetic energy of particles.
C) average potential energy of particles.
D) movement of energy from particle to particle.
E) none of the above
Answer: E
10) The fact that a thermometer "takes its own temperature" illustrates
A) thermal equilibrium.
B) energy conservation.
C) the difference between heat and thermal energy.
D) molecules are constantly moving.
Answer: A
11) Explain what is meant by saying a thermometer measures its own temperature.
Answer: Objects in the same locality will ultimately reach the same temperature when hot things
cool and cool things warm. This is what a thermometer does. Thermometers come to thermal
equilibrium with their surroundings and display this on their scale.
6.2 Absolute Zero
1) Which is the smallest unit of measurement for temperature?
A) one Celsius degree
B) one Kelvin
C) one Fahrenheit degree
D) all are the same
Answer: C
2) Absolute zero corresponds to a temperature of
A) 0 K.
B) -273° C.
C) both
D) neither
Answer: C
3) On which temperature scale is 0 degrees the freezing point of water?
A) Celsius
B) Caloric
C) Kelvin
D) Fahrenheit
E) none of the above
Answer: A
4) The lowest temperature possible in nature is
A) 0°C.
B) -273°C.
C) 4 K.
Answer: B
5) For each degree a volume of air at 0°C is cooled, its volume
A) shrinks by 1/273.
B) shrinks by 100/273.
C) increases by 1/273.
D) increases by 100/273.
Answer: A
6) For each degree a volume of air at 0°C is cooled, its pressure
A) decreases by 1/273.
B) decreases by 100/273.
C) increases by 1/273.
D) increases by 100/273.
Answer: A
7) At absolute zero, a substance has
A) absolutely no molecular motion.
B) no more energy to give up.
C) no volume.
D) all of the above
Answer: B
8) To say that something is twice as hot as another suggests the hotter thing has
A) twice the thermal energy.
B) twice the absolute temperature.
C) both
D) none of the above
Answer: A
9) A volume of helium gas has a temperature of 0°C. The same gas twice as hot has a
temperature of
A) 0°C.
B) 2°C.
C) 100°C.
D) 273°C.
E) none of the above
Answer: D
10) A volume of helium gas has a temperature of 10°C. The same gas twice as hot has a
temperature of
A) 10°C.
B) 12°C.
C) 283°C.
D) 293°C.
E) none of the above
Answer: D
6.3 Heat
1) Heat is simply another word for
A) temperature.
B) thermal energy.
C) thermal energy that flows from hot to cold.
D) radiant energy.
Answer: C
2) Heat energy is measured in units of
A) degrees.
B) joules.
C) calories.
D) both joules and calories.
Answer: D
3) Heat is thermal energy that flows due to
A) molecular activity.
B) calorie imbalance.
C) temperature differences.
Answer: C
4) Heat is thermal energy that flows from
A) hot to cold.
B) high energy to low energy.
C) high thermal pressure to low thermal pressure.
D) all of the above
Answer: B
5) Heat is thermal energy that matter
A) contains.
B) transfers.
C) both
D) none of the above
Answer: B
6) If a room is cold it is due to a
A) presence of cold air.
B) lack of adequate thermal energy.
C) low air pressure.
Answer: B
7) If the same quantity of heat is added to both a 1-liter and a 2-liter container of water, the
temperature change of water in the 1-liter container will be
A) half.
B) more than half but less than twice.
C) twice.
D) none.
Answer: C
8) If the same quantity of heat is added to both a 2-liter and a 4-liter container of water, the
temperature change for water in the 4-liter container will be
A) half that of the 2-liter container.
B) more than half but less than twice.
C) twice that of the 2-liter container.
D) no change.
Answer: A
9) Compared to a giant iceberg, a hot cup of coffee has
A) more thermal energy and higher temperature.
B) higher temperature, but less thermal energy.
C) a greater specific heat capacity and more thermal energy.
D) none of the above
Answer: B
10) The white-hot sparks from a fireworks sparkler that strike your skin don't cause injury
because
A) they have a low temperature.
B) the energy per molecule is very low.
C) the energy per molecule is high, but the total energy transferred is small.
Answer: C
11) Distinguish between the concepts of thermal energy, temperature, and heat.
Answer: Thermal energy, measured in calories or joules, is the energy something has by virtue of
the molecular motion of its molecules. The more molecular kinetic energy, the more thermal
energy. Temperature is this kinetic energy per molecule in a substance, measured in degrees (or
kelvins). Heat is thermal energy in transit; the thermal energy that transfers from one place to
another by virtue of a temperature difference. Heat, like thermal energy, is measured in calories
or joules.
6.4 Quantity of Heat
1) Thermal energy can be measured in
A) calories.
B) Calories.
C) joules.
D) any or all of the above for special cases
Answer: D
2) A nutritionist in the United States measures the food energy in units of
A) calories.
B) Calories.
C) joules.
D) none of the above
Answer: B
3) Increasing the temperature of 50 grams of water by 1°C requires
A) 1 calorie.
B) 50 calories.
C) none of the above
Answer: B
4) Pour a liter of 40°C water at into a liter of 20°C water and the final temperature of the two
liters becomes
A) less than 30°C.
B) at or about 30°C.
C) more than 30°C.
Answer: B
5) Place a 1-kg iron block at 40°C into 1 kg of water at 20°C and the final temperature becomes
A) less than 30°C.
B) at or about 30°C.
C) more than 30°C.
Answer: A
6) The temperature of water rises when 2.00 calories are added. It will rise the same when
A) 4.19 J are added.
B) 8.38 J are added.
C) 83.4 J are added.
Answer: B
7) A piece of iron and a cup of water both have the same temperature. If they are heated so the
thermal energy of each doubles,
A) the water will have the higher temperature.
B) the iron will have the higher temperature.
C) both will have the same temperature.
D) not enough information
Answer: B
6.5 The Laws of Thermodynamics
1) Which law of thermodynamics is a restatement of the conservation of energy as it applies to
thermal systems?
A) first law
B) second law
C) third law
D) all of the above
Answer: A
2) Which law of thermodynamics states that no system can reach absolute zero?
A) first law
B) second law
C) third law
D) all of the above
Answer: C
3) Which law of thermodynamics addresses the direction of heat flow?
A) first law
B) second law
C) third law
D) all of the above
Answer: B
4) When work is done on a system and no heat is added, the temperature of the system
A) increases.
B) decreases.
C) remains unchanged.
Answer: A
5) When work is done by a system and no heat is added, the temperature of the system
A) increases.
B) decreases.
C) remains unchanged.
Answer: B
6) When you place a sealed can of air on a hot stove burner, the can undergoes an increase in
A) thermal energy.
B) temperature.
C) pressure.
D) all of the above
E) none of the above
Answer: D
7) Suppose you rapidly stir some raw eggs with an egg beater. The temperature of the eggs will
A) increase.
B) decrease.
C) remain unchanged.
Answer: A
8) Because a refrigerator operates with some kind of motor, leaving the refrigerator door open in
a closed room on a hot day
A) increases room temperature.
B) decreases room temperature.
C) doesn't affect room temperature.
Answer: A
6.6 Entropy
1) The direction of natural processes is from states of
A) higher order to lower order.
B) lower order to higher order.
C) disorganization to organization.
D) imbalance to equilibrium.
Answer: A
2) As entropy in a system increases, energy within the system
A) becomes more ordered.
B) becomes less ordered.
C) reaches equilibrium.
D) moves toward destruction.
Answer: B
3) More disorder means
A) more entropy.
B) no real change in entropy.
C) less entropy.
Answer: A
4) As a system becomes more disordered, entropy
A) increases.
B) decreases.
C) remains the same.
Answer: A
5) Your room gets messier day by day. In this case entropy is
A) increasing.
B) decreasing.
C) hanging steady.
D) none of the above
Answer: A
6) Entropy is most closely related to the
A) first law of thermodynamics.
B) second law of thermodynamics.
C) both
D) neither
Answer: B
6.7 Specific Heat Capacity
1) The filling of a hot apple pie is hotter than the crust due to
A) water in the filling that better retains thermal energy.
B) uneven temperatures.
C) high conductivity of apples.
Answer: A
2) To say that water has a high specific heat capacity is to say that water
A) requires a lot of energy for an increase in temperature.
B) releases a lot of energy in cooling.
C) absorbs a lot of energy for an increase in temperature.
D) all of the above
Answer: D
3) A substance that heats up relatively quickly has a
A) high specific heat capacity.
B) low specific heat capacity.
C) high or low specific heat capacity.
Answer: B
4) Which of the following normally warms up faster when heat is applied?
A) water
B) iron
C) glass
D) wood
Answer: B
5) Which will cool faster when taken from a furnace?
A) iron
B) silver
C) the same
Answer: B
6) The moderate temperatures of islands throughout the world has mainly to do with water's
A) poor conductivity.
B) vast supply of thermal energy.
C) high specific heat capacity.
D) high evaporation rate.
E) absorption of solar energy.
Answer: C
7) San Francisco has milder winters than Washington D.C. due to water's high
A) conductivity.
B) specific heat capacity.
C) temperature in the Pacific Ocean.
Answer: B
8) The fact that desert sand is very hot in the day and very cold at night is evidence that sand has
a
A) low specific heat capacity.
B) high specific heat capacity.
C) none of the above
Answer: A
9) Hot sand cools off faster at night than plants and vegetation, which indicates that the specific
heat capacity for sand is
A) less than that for plants.
B) more than that for plants.
C) likely the same as that for plants.
D) not enough information
Answer: A
10) The specific heat capacity of aluminum is more than twice that of copper. Place equal masses
of aluminum and copper wire in a flame and the wire to heat up quickest will be
A) copper.
B) aluminum.
C) both the same
Answer: A
11) If the specific heat capacity of water were lower than it is, ponds in the cold of winter would
be
A) more likely to freeze.
B) less likely to freeze.
C) neither more nor less likely to freeze.
Answer: A
12) Some molecules are able to absorb large amounts of energy in the form of internal vibrations
and rotations. Materials composed of such molecules have
A) low specific heat capacities.
B) high specific heat capacities.
C) none of the above
Answer: B
13) What would be the temperature of a mixture of 50 g of 20°C water and 50 g of 40°C water?
A) 25°C
B) 28°C
C) 30°C
D) 32°C
E) 34°C
Answer: C
14) What would be the temperature of 50 g of 20°C water mixed with 80 g of 40°C water?
A) 24.6°C
B) 26.9°C
C) 27.6°C
D) 28.3°C
Answer: A
15) What would be the temperature of 40.0 g of 22°C water mixed with 60.0 g of 80°C water?
A) 28.4°C
B) 30.2°C
C) 50.6°C
D) 56.8°C
Answer: D
16) Place a kilogram block of iron at 40°C into a kilogram of water at 20°C and the final
temperature of the two becomes
A) less than 30°C.
B) at or about 30°C.
C) more than 30°C.
Answer: A
17) If water had a lower specific heat capacity, would ponds and lakes be more or less likely to
freeze in winter?
Answer: Bodies of water would more likely freeze, because the temperature would decrease
more as water loses energy, and the water would be more readily cooled to the freezing point.
6.8 Thermal Expansion
1) Which of the following expands most when the temperature is increased? Equal volumes of
A) iron.
B) wood.
C) ice water.
D) helium.
E) all expand the same
Answer: D
2) Which of the following expands most when the temperature is lowered? Equal volumes of
A) iron.
B) wood.
C) helium.
D) water at 4°C.
E) none expand when the temperature is lowered
Answer: D
3) Which of the following contracts most when the temperature is decreased? Equal volumes of
A) iron.
B) wood.
C) water.
D) helium.
E) all contract the same
Answer: D
4) Which of the following contracts most when the temperature is slightly increased? Equal
volumes of
A) iron.
B) wood.
C) ice water.
D) helium.
E) none of the above contract when heated
Answer: C
5) The usefulness of a bimetallic strip is due to differences in
A) expansions of metals.
B) conductivities of metals.
C) heat capacities of metals.
Answer: A
6) When a bimetallic bar composed of copper and iron strips is heated, the bar bends toward the
iron strip because
A) iron gets hotter before copper.
B) copper gets hotter before iron.
C) copper expands more than iron.
D) iron expands more than copper.
E) none of the above
Answer: C
7) A pre-electronic thermostat employs a coiled
A) wire of low conductivity.
B) bimetallic strip.
C) tube of mercury.
Answer: B
8) If glass expanded more than mercury, then the column of mercury in a thermometer would
rise when the temperature
A) increases.
B) decreases.
C) neither
Answer: B
9) When an iron ring is heated, the hole becomes
A) smaller.
B) larger.
C) neither
Answer: B
10) As a hot iron ring cools, the diameter of the hole
A) increases.
B) decreases.
C) remains the same.
Answer: B
11) A metal ring with a gap in it is shaped like the letter C. When heated, the gap becomes
A) wider.
B) narrower.
C) remains the same size.
Answer: A
12) A metal ring with a gap in it is shaped like the letter C. When the hot metal cools, the gap
becomes
A) wider.
B) narrower.
C) remains the same size.
Answer: B
13) During a very cold winter, water pipes sometimes burst because
A) the ground contracts when colder, pulling pipes apart.
B) water expands when freezing.
C) water contracts when freezing.
D) the thawing process releases pressure on the pipes.
E) none of the above
Answer: B
14) The overflow spillage of gasoline from a car's full tank on a hot day is evidence that gasoline
expands
A) more than the tank metal.
B) about the same as the tank metal.
C) less than the tank metal.
D) negligible.
Answer: A
6.9 Expansion of Water
1) The open spaces in the crystal lattice of ice contain
A) vapor.
B) trace amounts of water.
C) nothing.
Answer: C
2) If the temperature of a sample of 0°C water slightly increases, the sample of water
A) expands.
B) contracts.
C) neither
Answer: A
3) If the temperature of a sample of 4°C water slightly increases, the sample of water
A) contracts.
B) expands.
C) neither
Answer: B
4) If the temperature of a sample of 4°C water slightly decreases, the sample of water
A) contracts.
B) expands.
C) neither
Answer: B
5) Water at 4°C will expand when it is slightly
A) cooled.
B) warmed.
C) both
D) neither
Answer: C
6) Consider a sample of water at 20°C. If the temperature is slightly increased, the water
A) expands.
B) contracts.
C) remains the same.
Answer: A
7) Microscopic slush in water tends to make the water
A) more dense.
B) less dense.
C) slipperier.
D) warmer.
Answer: B
8) The greatest expansion of water occurs when
A) it turns to ice.
B) at 4°C it gains temperature.
C) at 4°C it loses temperature.
D) none of the above
Answer: A
9) The density of water at 4°C will slightly decrease when it is
A) cooled.
B) warmed.
C) both
D) neither
Answer: C
10) Water at 4°C will sink to the bottom of a pond because
A) it will not freeze there.
B) it benefits fish and other life forms there.
C) like a rock, it is denser than surrounding water.
D) of the presence of microscopic ice crystals.
Answer: C
11) Ice has a lower density than water because ice
A) sinks.
B) molecules are more compact in the solid state.
C) molecules vibrate at lower rates than water molecules.
D) is composed of open-structured crystals.
E) density decreases with decreasing temperature.
Answer: D
12) Before ice can form on a lake, all the water in the lake must be cooled to
A) 0°C.
B) 4°C.
C) a value slightly below 0°C.
Answer: B
13) Ice tends to form at the
A) surface of bodies of water.
B) layer of water slightly below the surface.
C) bottom of bodies of water.
Answer: A
14) The temperature at the bottom of Lake Tahoe, high in the Sierra Mountains in California, at
this moment is
A) below 4°C.
B) 4°C.
C) above 4°C.
D) uncertain.
Answer: B
15) When ice floats in water, a small part of it extends above the surface. Interestingly, the
volume of ice that extends above the surface is equal to the volume of the
A) water the ice displaces.
B) vast number of open spaces in the hexagonal ice crystals.
C) both
D) neither
Answer: B
16) Write a short paragraph explaining why fish live through cold winters even when the ponds
are frozen over.
Answer: Water has its greatest density at 4°C. So water in a lake that reaches 4°C sinks to the
bottom, just as anything else denser than water will sink in water. This results in a 4 °C water
temperature at the bottom of a lake in cold climates. Since water is a poor conductor of heat, the
4°C water persists year-round unless the lake is shallow. Fish survive in cold winters in this 4 °C
water. Only in shallow waters will freezing be complete to the bottom. Then fish are in trouble!
Test Bank for Conceptual Physical Science
Paul Hewitt, John Suchocki, Leslie Hewitt
9780321752932, 9780134060491
