Ch.12 physics test practice questions

Heat tends to flow from the ____________________ object to the ____________________ object.

Warmer, colder

The temperature at which a liquid changes into a gas is called the __________________.

Boiling point

To melt 4 kg of a solid, 10^6 J of heat is required. Which of the following expressions gives the heat of fusion of the solid?

C. 10^6/4 j/kg

The volume of a gaseous system increases when it does positive work in a thermodynamic process

True

Thermal equilibrium occurs when two objects have the same temperature

True

A 50.0 g ice cube is at its melting point. How much thermal energy is absorbed for it to become water at room temperature (17ºC)?

C. 2.03 x 10^4 J

Which is not a correct temperature equivalent?

C. 289ºC=552K

A man has a metabolic rate of 150 W when he is working on a computer. Assuming he has a normal body temperature of 37C, calculate the rate at which his entropy is changing.

-0.48 J/K•s

On the Celsius scale, the freezing point of pure water is defined as ___________________.

0º C

A 3.00 10-3-kg lead bullet enters a target with a speed of 2.00 102 m/s and comes to rest within the target. Calculate the rise in temperature of the bullet assuming that 80.0% of the heat produced is absorbed by the bullet. The specific heat of lead is 1.30 102 J/kg K.

123k

A 0.10-kg copper calorimeter contains 0.15 kg of paraffin at 15.0C. When a 0.050-kg piece of aluminum at 100.0C is dropped into the calorimeter, the final temperature of the mixture is 25.0C. Calculate the specific heat capacity of paraffin. The specific heat capacities of aluminum and copper are 1.0 103 J/kg K and 4.0 102 J/kg K respectively.

2.2 x 10^3 J/kg•K

A 0.200-kg piece of lead at 100.0C is dropped into a calorimeter. The calorimeter is a copper can of mass 5.00 10-2 kg and already contains 0.100 kg of water at 20.0C. Calculate the final temperature if the specific heats of water, lead, and copper are 4.20 103 J/kg K, 1.30 102 J/kg K, and 4.00 102 J/kg K respectively.

24.5 ºC

Calculate the change in entropy of 0.020 kg of ice when it melts at 0.0C. The heat of fusion of ice is 3.36 105 J/kg.

25 J/K

The normal atmospheric boiling point of water is ____________________ Kelvin.

373

How much heat must be removed from 0.15 kg of water to cool it from 95C to 25C? The specific heat capacity of water is 4182 J/kg K.

4.4 x 10^4 J

The temperature of a 2-kg metal block rises by 10C when 8000 J is supplied to it. What is the specific heat of the metal?

400 J/kg ºC

Convert 173ºC to kelvins

446K

The temperature of a 0.0020-kg of fusion of bullet is 0.0C. The material of the bullet has a specific heat of 840 J/kg K and a heat of fusion of 6.3 104 J/kg. What is the minimum velocity with which the bullet should be fired for it to melt completely when suddenly brought to rest? The bullet melts at 400.0C. Assume that the kinetic energy is completely converted to heat and there is no loss of heat.

890 m/s

A 0.050-kg copper calorimeter contains 0.050 kg of ice at -10.0C. What mass of steam at 100.0C is required to convert the ice to water at 30.0C? Specific heat capacity of ice = 2.1 103 J/kg Specific heat capacity of water = 4.2 103 J/kg Specific heat capacity of copper = 4.0 102 J/kg Specific latent heat of fusion of ice = 3.36 105 J/kg Specific latent heat of vaporization of water = 2.25 106 J/kg

9.8 x 10^-3 Kg

Explain why the air that comes out of a burst tire is cooler than the surrounding air.

A tire burst is a sudden change and there is not much heat transfer. The expanding air does positive work. According to the first law of thermodynamics, this work causes an equal decrease in internal energy. The decrease in internal energy relates to a decrease in the average kinetic energy of the molecules and, therefore, the temperature.

A block of copper (specific heat = 385 J/kg•K) requires 635,000 J of thermal energy to change in temperature from 17C to 139C. What is the mass of this copper block?

A. 13.5 kg

A 2.15 kg block of aluminum (specific heat = 897 J/kg•K) is at an initial temperature of 300 K. What will its final temperature be if 335,000 J of thermal energy are added?

A. 260K; 335,000 J = 2.15 kg • 897 J/kg•K • (Tf -300) Tf=474k

How much thermal energy is required to completely melt 10.6 kg of ice at its melting point?

A. 3.54 x 10^6 J

5000 J of heat is supplied in one minute to 0.06 kg of a liquid at its boiling point of 85°C to convert it completely to vapor. Which of the following expressions gives the heat of vaporization of the liquid?

A. 5000/0.06 J/kg

How much thermal energy is released when 2.75 kg of steam is completely condensed?

A. 6.22 x 10^6 J

Which of the followings physical properties can be used to measure temperature using a thermometer?

A. Volume

Which is an example of heating through convection?

A. Warm air rising toward the ceiling ;Heating through convection occurs through the circulation of warm liquids and gases.

Which is the transfer of thermal energy through direct contact of particles?

A. conduction; Conduction is the transfer of thermal energy through direct contact of particles.

What happens when water at its melting point solidifies to ice without any change in temperature?

A.latent heat is emitted

93.Compare the behavior of solids and gases on the particle level as these substances heat up.

As an object heats up, its particles have an increased amount of kinetic and potential energies. Particles in solids remain connected to one another, as if by springs. Their increased energy results in an increased vibration of these particles between one and another. Gases, however, are only loosely connected to one another and are free to move. Increased heat results in these particles gaining kinetic energy that causes them to both move faster and collide more frequently. This results in larger changes in volume for gases as temperatures change.

A total of 95,000 J of thermal energy are added to 2.81 kg of lead (specific heat = 130 J/kg•K) to reach a final temperature of 642 K. What was the initial temperature of the lead?

B. 382K; 95,000 J = 2.81 kg • 130 J/kg•K • (642 K-Ti) Ti=382k

Thermodynamic values for water: heat of fusion = 3.34 x. 10^5 J/kg heat of vaporization = 2.26x106 J/kg specific heat = 4180 J/kg K How much thermal energy is required to completely boil 2.83 kg of water from an initial temperature of 50ºC?

B. 5.80 x 10^6 J

When a closed tin is heated, the pressure inside it increases. This happens because:

B. The molecules move faster and each molecule strikes the walls of the tin more often

Which is an example of heating through conduction?

B. Touching a hot stove; when you touch a hot stove, you rapidly heat your hand through conduction.

The melting point of a solid is 90.0ºC. What is the heat required to change 2.5 kg of this solid at 40.0ºC to a liquid? The specific heat of the solid is 390 J/kg K and its heat of fusion is 4000 J/kg.

C. 5.9 x 10^4 J

A solid is heated at a constant rate until it reaches the vapor state. The temperature of the substance changes with time as shown in the graph below. Which part(s) of the graph indicate(s) that the substance exists in solid-liquid and liquid-vapor state? (There is a graph but I can't even put it in it)

C. PQ, RS

Which type of change requires more energy for the same substance?

C. Vaporizing into a gas

Which is the transfer of thermal energy through the motion of particles caused by temperature differences?

C. convection; thermal energy transferred by the motion of particles of particles is called convection

The total amount of thermal energy is constant in a ___________________.

Closed system

The specific heat of copper is 385 J/kg•K. If a 2.6 kg block of copper is heated from 300 K to 450 K, how much thermal energy is absorbed?

D. 150,000 J; a=2.6 kg • 385 J/kg•K • (450 K 350 K) = 150,000 J

50 g of ice at 0°C is dropped in a beaker containing 100 g of water at 0°C. What will be the contents of the beaker after 5 hours? Assume that the room temperature is 0°C.

D. 50g of ice and 100g of water

What is the specific heat of a substance that requires 99,100 J of thermal energy to heat 3.47 kg of this substance from 11ºC to 45ºC?

D. 840 J/kg•K

Which is not associated with an increase in entropy?

D. a more orderly arrangement of particles

The ratio of useful work produced compared to the amount of input heat is referred to as____________________.

Efficiency

Compare and contrast warm-blooded animals (endotherms) with cold-blooded animals (ectotherms).

Endotherms regulate their body temperature by changing their metabolic rate to maintain a constant internal temperature. Ectotherms' internal temperatures change to reflect the temperature of their environment.

The measure of disorder in a system is called ____________________.

Entropy

A hot object has more thermal energy than a similar cold object only because of greater kinetic energy.

False; A hot object has more thermal energy than a similar cold object because of greater kinetic energy and potential energy.

Absolute zero is defined as the zero point on trey Celsius scale.

False; Absolute zero is defined as the zero point on the Kelvin scale.

Some machines can accomplish work with no increase in entropy because they have no friction associated with them

False; Every machine increase entropy when it does work

In a vacuum flask, the vacuum helps in reducing heat loss due to radiation.

False; Heat transfer can take place through vacuum by the process of radiation. A vacuum does not allow heat transfer by conduction and convection

The thermal energy of the p[articles in a gas is related to the temperature of the gas

False; The average energy per particle is related to the temperature of the gas and not the thermal energy which is the total energy of the particles

When the same amount of thermal energy is added to both an object with high specific heat and an object with low specific heat , the object with a high specific heat will increase in temperature more than the object with a low specific heat.

False; The object with a high specific heat will increase in temperature less than an object with low specific heat.

The temperature of a bottle containing water rises when it is shaken vigorously since shaking adds heat to the system

False; The temperature rises because work is done on the system. No heat is added.

Thermal equilibrium is the point at which no more thermal energy. Is transferred between objects

False; Thermal energy continues to transfer between objects at thermal equilibrium, but there is no net thermal energy transfer.

A heat pump works because it does not have to obey the second law of thermodynamics.

False; a heat pump requires mechanical energy to remove heat from an area

Entropy it's the amount of work done in the absence of friction

False; entropy is a measure of disorder in a system

The amount of thermal energy transferred between objects depends only on their masses and initial and final temperatures

False; specific heat is also a factor

Mechanical energy can be converted to thermal energy through friction, but the reserve never occurs

False; with difficulty, thermal energy can be converted to mechanical energy

The temperature of a system must increase when heat energy is added.

False;A system can maintain its temperature by doing work equal to the amount of heat added, or the system can undergo a change in state.

The ____________________ law of thermodynamics explains that energy cannot be created or destroyed.

First; the first law of thermodynamics is the same as the law of conservation of energy

The amount of energy required to melt a solid depends on its mass and its ____________________

Heat of fusion

The amount of energy required to vaporize a liquid depends on its mass and its____________________.

Heat of vaporization

94.Explain why the heat of vaporization is greater than the heat of fusion for most substances.

It requires more energy to vaporize a liquid at its boiling point because the particles have to overcome additional forces attracting particles to one another in order for the particles to vaporize. Melting a solid does not take as much energy because although the particles are no longer in a regular arrangement as in the solid phase, they have more forces holding them in the liquid phase.

James places a 100 g block of copper at 50C next to a 100 g block of silver at 20C. He asserts that at thermal equilibrium, the final temperatures of both blocks of metal will be 35C. Do you agree with James? Explain why or why not.

James is incorrect. The final temperature depends on the specific heat of the each substance. Since the silver has a lower specific heat, it will change in temperature more than the copper as thermal energy is exchanged.

During heating, added thermal energy is used to increase the motion or ____________________ of particles.

Kinetic energy

The temperature at which a substance changes from a solid into a liquid is called the __________________.

Melting point

When heat is transferred out of an object, the sign of its value for Q is_________________.

Negative

92. Propose an experimental design that would allow you to determine the identity of an unknown metal using thermodynamics concepts.

One could use specific heat to identify a metal by using calorimetry to determine the specific heat of the metal and looking up the specific heat value in a data table. The metal should be heated to a known initial temperature, perhaps by immersing it in boiling water for approximately 5-10 minutes. It can then be placed into a known mass of water at a known initial temperature in a well-insulated container. The final temperature of the water should be determined after the system reaches thermal equilibrium. The change in thermal energy of the water will be equal to the thermal energy change of the metal; the sum of the two thermal energies will be zero, allowing one to calculate the specific heat value of the metal.

A piece of copper (specific heat = 385 J/kg•K) has a mass of 275 g. If it is heated to 145C, then plunged into 5.00 kg water (specific heat = 4180 J/kg•K) at 20C, what will be the final temperature at equilibrium?

Qa+Qb = 0 (0.275 kg)(385 J/kg•K)(Tf 145C) + (5.00 kg)(4180 J/kg•K)(Tf 20C) = 0 105.875Tf 15351.875 + 20900 418000 21005.88 Tf = 433351.9 Tf = 20.6C

The ____________________ law of thermodynamics explains that the amount of entropy in a system tends to increase.

Second; entropy increase whenever work is done, according to the second law of thermodynamics

90. Find the amount of energy required to change a 4.50 kg block of ice at the temperature, shown by point a on the graph, to a liquid at the temperature shown by point d on the graph

Step 1: Q = mC( ); Q = (4.50 kg)(2060 J/kgK)(273 150) = 1140210 J Step 2: Q = mHf = (4.50 kg)(3.34 105 J/kg) = 1,503,000 J Step 3: Q = mC( ); Q = (4.50 kg)(4180 J/kgK)(320 273) = 884,070 J Total = 3,527,280 = 3.53 106 J

91. Find the amount of energy required to change a 4.50 kg block of ice just at its melting point to a gas at the temperature shown by point g on the graph.

Step 1: Q = mHf = (4.50 kg)(3.34 105 J/kg) = 1,503,000 J Step 2: Q = mC( ); Q = (4.50 kg)(4180 J/kgK)(373 273) = 1,881,000 J Step 3: Q = mHf = (4.50 kg)(2.26 106 J/kg) = 10170000 J Step 4: Q = mC( ); Q = (4.50 kg)(2020 J/kgK)(500 373) = 1,154,430 J Total = 13,205,430 = 1.32 107 J

James states that the Second Law of Thermodynamics is violated when plants grow, because the mature plant is more organized. Do you agree with James? Explain your response.

The Second Law of Thermodynamics is not violated. It applies to a closed system, and in the case of a plant growing, one needs to take into account the energy input from the Sun.

What is the change in the internal energy of a gaseous system in a cyclic process?

The internal energy does not change in a cyclic process

When heat flows into an object, it's temperature and thermal energy increase.

True

A fixed mass of a gas at a temperature T is present in a container. Exactly half the molecules of the gas are removed from the container without changing the average kinetic energy per molecule of the gas within the container. What is the temperature of the gas still in the container?

The temperature of the gas in the container is T

95.Explain how a refrigerator can continue to keep food cold if warmer food continues to be added to it.

Thermal energy flows spontaneously to the air in the refrigerator from the warmer food, cooling the food down. In order to keep the air in the refrigerator cold, energy must be removed from it. Pipes circulate in the refrigerator and contain a liquid that is vaporized as thermal energy is removed from the inside of the refrigerator. The gas passes through a condenser where thermal energy is removed from the gas, converting it to a liquid, and releasing the thermal energy to the air outside the refrigerator.

The point at which the net flow of thermal energy between two objects at the same temperature is zero is called ___________________.

Thermal equilibrium; at this between two objects, the net flow of thermal energy between those objects is zero

The study of heat transformations into other forms of energy is called____________________.

Thermodynamics

Explain why the heat of fusion and heat of vaporization do not depend on a substance's temperature.

These do not depend on temperature because they occur at a set temperature, either the melting point or boiling point respectively.

A machine can never be 100 percent efficient because some energy is lost as waste heat.

True

An insulated cooler has held a mixture of ice and water all day. The temperature of the water and the temperature of the ice are therefore the same.

True

During melting or vaporization, particles increase in potential energy but not in kinetic energy

True

In thermodynamics terms, a sink where the thermal energy is deposited

True

It is not possible to have a process in which the entropy of an isolated system decreases

True

Refrigerators work because the heat flows spontaneously from warmer food to the colder air inside the refrigerator

True

The entropy of a system measures the state of disorder of the system

True

The magnitude of one degree Celsius is the same as one Kelvin

True

0.2000 kg of water at 20.00C is contained in a 0.1000-kg copper container. The container is shaken vigorously for 10.00 minutes to cause the temperature to rise to 22.00C. Calculate the work done on the system and the heat supplied to the system. The specific heat of copper is 385.0 J/kg K and of water is 4200.0 J/kg K.

Work done =1757J Heat supplied=0

A gas is kept in a rigid container and 100 J of heat is supplied to it. What is the work done by the gas and the change in the internal energy of the gas?

Work done by the gas =0J Change in internal energy =-100J