Ch. 9 & 10
How is energy transferred as heat always directed?
from an object at high temperature to an object at low temperature
Which of the following terms describes a transfer of energy?
heat
What thermodynamic process for an ideal gas system has an unchanging internal energy and a heat intake that corresponds to the value of the work done by the system?
isothermal
Which thermodynamic process takes place at a constant temperature so that the internal energy of a system remains unchanged?
isothermal
Which thermodynamic process takes place at constant volume so that no work is done on or by the system?
isovolumetric
Energy transferred as heat occurs between two bodies in thermal contact when they differ in which of the following properties?
temperature
Which of the following is proportional to the kinetic energy of atoms and molecules?
temperature
At what point on the figure above is the amount of energy transferred as heat approximately 4.19 ¥ 103 J?
C
When a sample of water at 0.0°C is cooled to -36.0°C and freezes in the process, 935,000 kJ of heat is liberated. What is the mass of this sample of water?
2290 kg
A fixed amount of an ideal monatomic gas is maintained at constant volume as it is cooled by 50 K. This feat is accomplished by removing 400 J of energy from the gas. How much work is done by the gas during this process?
0 J
An ideal gas system is maintained at a constant volume of 4 L. If the pressure is constant, how much work is done by the system?
0 J
An ideal gas system undergoes an adiabatic process in which it expands and does 20 J of work on its environment. How much energy is transferred to the system as heat?
0 J
During an isothermal process, 5.0 J of heat is removed from an ideal gas. What is the change in internal (thermal) energy of the gas?
0 J
The work done on an ideal gas system in an isothermal process is -400 J. What is the change in internal (thermal) energy of the gas?
0 J
A monatomic ideal gas undergoes an isothermal expansion at 300 K, as the volume increased from 0.010 m^3 to 0.040 m^3. The final pressure is 130 kPa. What is the change in the internal (thermal) energy of the gas during this process? (R = 8.31 J/mol • K)
0.0 kJ
An athlete doing push-ups performs 650 kJ of work and loses 425 kJ of heat. What is the change in the internal (thermal) energy of the athlete?
-1075 kJ
The gas in a perfectly insulated but flexible container does work at a rate of 13 W. At what rate is the internal (thermal) energy of the gas changing?
-13 W
A compression at a constant pressure of 200 kPa is performed on 8.00 moles of an ideal monatomic gas. The compression reduces the volume of the gas from 0.200 m^3 to 0.120 m^3. How much work was done by the gas during this process?
-16 kJ
An ideal gas system undergoes an adiabatic process in which it expands and does 20 J of work on its environment. What is the change in the system's internal energy?
-20 J
An ideal gas undergoes an adiabatic process while doing 25 J of work. What is the change in the internal (thermal) energy of the gas?
-25 J
During an isothermal process, 5.0 J of heat is removed from an ideal gas. What is the work done by the gas in the process?
-5.0 J
A nuclear power plant has an actual efficiency of 33%. If .19 MW of energy are released from fission, how much electric power does the power plant produce?
0.063 MW
A steel bridge is 1000 m long at -20°C in winter. What is the change in length when the temperature rises to 40°C in summer? The average coefficient of linear expansion of this steel is 11 ¥ 10-6 K-1.
0.66 m
By what length will a slab of concrete that is originally 18 m long contract when the temperature drops from 24°C to -16°C? The coefficient of linear thermal expansion for this concrete is 1.0 ¥ 10-5 K-1.
0.72 cm
An aluminum rod is 10.0 cm long and a steel rod is 80.0 cm long when both rods are at a temperature of 15°C. Both rods have the same diameter. The rods are now joined end-to-end to form a rod 90.0 cm long. If the temperature is now raised from 15°C to 90°C, what is the increase in the length of the joined rod? The coefficient of linear expansion of aluminum is 2.4 ¥ 10-5 K-1 and that of steel is 1.2 ¥ 10-5 K-1.
0.90 mm
Which two temperature changes are equivalent?
1 C° = 1 K
The coefficient of linear expansion of steel is 12 ¥ 10-6 K-1. What is the change in length of a 25-m steel bridge span when it undergoes a temperature change of 40 K from winter to summer?
1.2 cm
A hole in a brass plate has a diameter of 1.200 cm at 20°C. What is the diameter of the hole when the plate is heated to 220°C? The coefficient of linear thermal expansion for brass is 19 ¥ 10-6 K-1.
1.205 cm
When 50 g of a certain material at 100°C is mixed with 100 g of water at 0°C, the final temperature is 40°C. What is the specific heat of the material? The specific heat of water is 1.00 kcal/kg • C°.
1.3 kcal/kg • C°
A 45.0-kg sample of ice is at 0.00° C. How much heat is needed to melt it?
1.50 X 10^4 kJ
Heat is added to a 3.0 kg piece of ice at a rate of How long will it take for the ice at 0.0° C to melt?
1.6 s
What is the temperature of a system in thermal equilibrium with another system made up of water and steam at 1 ATM of pressure?
100°C
The figure shows a pV diagram for an ideal gas that is carried around a cyclic process. How much work is done in one cycle if p0 = 4.00 ATM v0 = 3.00 and L? (1.00 atm = 101 kPa) Hint: What is the area of the enclosed space?
1210 J
A .20-kg ice cube at 0.0°C has sufficient heat added to it to cause total melting, and the resulting water is heated to 70 degrees Celsius. How much heat is added?
130 kJ
At room temperature, a typical person loses energy to the surroundings at the rate of 62 W. If this energy loss has to be made up by an equivalent food intake, how many kilocalories (food calories) does this person need to consume every day just to make up this heat loss? (1 cal = 4.186 J)
1300 kcal
A lab student drops a 400.0-g piece of metal at 120.0°C into a cup containing 450.0 g of water at 15.0°C. After waiting for a few minutes, the student measures that the final temperature of the system is 40.0°C. What is the specific heat of the metal, assuming that no significant heat is exchanged with the surroundings or the cup? The specific heat of water is 4186 J/kg • K.
1470 J/kg • K
An aluminum rod 17.400 cm long at 20°C is heated to 100°C. What is its new length? Aluminum has a linear expansion coefficient of 25 ¥ 10-6 K-1.
17.435 cm
If you add 1.33 MJ of heat to 500 g of water at 50°C in a sealed container, what is the final temperature of the steam? The latent heat of vaporization of water is 22.6 ¥ 105 J/kg, the specific heat of steam is 2010 J/kg • K, and the specific heat of water is 4186 J/kg • K.
195°C
A 44.0-g block of ice at -15.0°C is dropped into a calorimeter (of negligible heat capacity) containing 100 g of water at 5.0°C. When equilibrium is reached, how much of the ice will have melted? The specific heat of ice is 2090 J/kg • K, that of water is 4186 J/kg • K, and the latent heat of fusion of water is 33.5 ¥ 104 J/kg.
2.1 g
A person consumes a snack containing 14 food calories (14 kcal). What is the power this food produces if it is to be "burned off" due to exercise in 6 hours? (1 cal = 4.186 J)
2.7 W
An ideal gas system undergoes an isovolumetric process in which 20 J of energy is added as heat to the gas. What is the change in the system's internal energy?
20 J
A substance registers a temperature change from 20°C to 40°C. To what incremental temperature change does this correspond?
20 K
In an adiabatic compression, 200 J of work is done on a gas. What is the change in internal (thermal) energy of the gas during this compression?
200 J
How much heat must be removed from 456 g of water at 25.0°C to change it into ice at -10.0°C? The specific heat of ice is 2090 J/kg • K, the latent heat of fusion of water is 33.5 ¥ 104 J/kg, and the specific heat of water is 4186 J/kg • K.
210 kJ
A 400-g block of iron at 400°C is dropped into a calorimeter (of negligible heat capacity) containing 60 g of water at 30°C. How much steam is produced? The latent heat of vaporization of water is 22.6 ¥ 105 J/kg and its specific heat capacity is 4186 J/kg • K. The average specific heat of iron over this temperature range is 560 J/kg • K.
22 g
Using the figure above, determine which value equals the latent heat required to change the liquid water into steam.
22.6 X 103 J
A lab assistant drops a 400.0-g piece of metal at 100.0°C into a 100.0-g aluminum cup containing 500.0 g of water at 150 degrees Celsius. In a few minutes, she measures the final temperature of the system to be 40.0°C. What is the specific heat of the 400.0-g piece of metal, assuming that no significant heat is exchanged with the surroundings? The specific heat of this aluminum is 900.0 J/kg • K and that of water is 4186 J/kg • K.
2270 J/kg • K
A substance has a melting point of 20°C and a heat of fusion of 3.4 X 10^4 J/kg. The boiling point is 150 degrees Celsius and the heat of vaporization is 6.8 X 10^4 J/kg at a pressure of one atmosphere. The specific heats for the solid, liquid, and gaseous phases are 600 J/kg • K (solid), 1000 J/kg • K (liquid), and 400 J/kg • K (gaseous). How much heat is required to raise the temperature of 1.90 kg of this substance from -4 degrees Celsius to at a pressure of one atmosphere?
260 kJ
What is the temperature of a system in thermal equilibrium with another system made up of ice and water at 1 ATM of pressure?
273 K
How much heat is required to raise the temperature of a 225-g lead ball from 15.0°C to 25.0°C? The specific heat of lead is 128 J/kg • K.
288 J
A person running in place on an exercise machine for 10 min uses up 17 kcal (food calories). Another person exercises by repeatedly lifting two 2.5-kg weights a distance of 50 cm. How many repetitions of this exercise are equivalent to 10 minutes of running in place? Assume that the person uses negligible energy in letting down the weights after each lift. (1 cal = 4.186 J)
2900
The temperature in your classroom is closest to
295 K.
A gas is taken through the cycle shown in the pV diagram in the figure. During one cycle, how much work is done by the gas?
3 p0V0
The figure shows a graph of the temperature of a pure substance as a function of time as heat is added to it at a constant rate in a closed container. If LF is the latent heat of fusion of this substance and LV is its latent heat of vaporization, what is the value of the ratio LV/LF?
3.5
A gas expands from an initial volume of 30.0 L to a final volume of 65.0 L at a constant pressure of 110 kPa. How much work is done by the gas during this expansion?
3.85 kJ
A lab assistant pours 330 g of water at 45°C into an 855-g aluminum container that is at an initial temperature of 10°C. The specific heat of aluminum is 900 J/kg X k and that of water is 4186 J/kg • K. What is the final temperature of the system, assuming no heat is exchanged with the surroundings?
32°C
A 920-g empty iron kettle is put on a stove. How much heat in joules must it absorb to raise its temperature form 15 degrees Celsius to 93 degree Celsius. The specific heat for iron is 113 cal/kg • C°, and 1 cal = 4.186 J.
33,900 J
An ideal gas undergoes the process a-b-c-a shown in the pV diagram. In this figure, Pa = Pc = 3.60 X 10^5 Pa, Vb = Vc = 68.00 L, Va = 35 L, and Pb = 5.60 X 105 Pa. How much work is done by the system in this process? Convert volumes to m3
3300 J
A 35-g block of ice at -14°C is dropped into a calorimeter (of negligible heat capacity) containing 400 g of water at 0°C. When the system reaches equilibrium, how much ice is left in the calorimeter? The specific heat of ice is 2090 J/kg • K
38 g
A fluid in an insulated, flexible bottle is heated by a high resistance wire and expands. If 9.0 kJ of heat is applied to the system and it does 5.0 kJ of work, how much does the internal (thermal) energy of the fluid change?
4.0 kJ
A 771.0-kg copper bar is put into a smelter for melting. The initial temperature of the copper is 300.0 K. How much heat must the smelter produce to completely melt the copper bar? The specific heat for copper is 386 J/kg•K, the heat of fusion for copper is 205,000 J/kg, and its melting point is 1357 K.
4.73 X 10^5 kJ
A substance has a melting point of 20°C and a heat of fusion of 3.6 X 10^4 J/kg. The boiling point is 150 degrees Celsius and the heat of vaporization is 7.2 X 10^4 J/kg at a pressure of one atmosphere. The specific heats for the solid, liquid, and gaseous phases are 600 J/kg • K (solid), 1000 J/kg • K (liquid), and 400 J/kg • K (gaseous). How much heat is given up by 2.8 kg of this substance when it is cooled from 170°C to 86°C at a pressure of one atmosphere?
400 kJ
A certain heat engine extracts 1.30 kJ of heat from a hot temperature reservoir and discharges 0.70 kJ of heat to a cold temperature reservoir. What is the efficiency of this engine?
46%
A 90-g aluminum calorimeter contains 390 g of water at an equilibrium temperature of 20 degrees celcius. A 160 g piece of metal, initially at 305 degrees celcius is added to the calorimeter. The final temperature at equilibrium is 32° C. Assume there is no external heat exchange. The specific heat capacities of aluminum and water are 910 J/kg • K (aluminum) and 4190 J/kg • K (water). What is the specific heat capacity of the 160-g piece of metal?
470 J/kg • K
The melting point of aluminum is 660°C, its latent heat of fusion is 4.00 ¥ 105 J/kg, and its specific heat is 900J/kg • K. How much heat must be added to 500 g of aluminum originally at 27°C to completely melt it?
485 kJ
A runner generates 1260 W of thermal energy. If this heat has to be removed only by evaporation, how much water does this runner lose in 15 minutes of running? The latent heat of vaporization of water is 22.6 ¥ 105 J/kg.
500 g
A 40.0-g block of ice at -15.00°C is dropped into a calorimeter (of negligible heat capacity) containing water at 15.00°C. When equilibrium is reached, the final temperature is 8.00°C. How much water did the calorimeter contain initially? The specific heat of ice is 2090 J/kg • K, that of water is 4186 J/kg • K, and the latent heat of fusion of water is 33.5 ¥ 104 J/kg.
546 g
A 4.0-kg aluminum block is originally at 10°C. If 160 kJ of heat is added to the block, what is its final temperature? The specific heat capacity of aluminum is 910 J/kg • K.
54°C
An external heat source supplies heat to a system at a rate of 187 W as the system does work at a rate of 131 W. At what rate is the internal (thermal) energy of the system changing?
56 W
A heat engine receives 7000 J of heat and loses 3000 J in each cycle. What is the efficiency of this engine?
57%
A heat engine with an efficiency of 30% performs 2500 J of work. How much heat is discharged to the lower temperature reservoir? First find the amount of heat added to the system.
5800 J
A 200-L electric water heater uses 2.0 kW. Assuming no heat loss, how many hours would it take to heat the water in this tank from 23°C to 75°C? The specific heat of water is 4186 J/kg • K and its density is 1000 kg/m3.
6.0 hours
If 50 g of lead (of specific heat 0.11 kcal/kg • C°) at 100°C is put into 75 g of water (of specific heat 1.0 kcal/kg • C°) at 0°C. What is the final temperature of the mixture?
6.8°C
A steel pipe 36.0 m long, installed when the temperature was 15 degree Celsius is used to transport super heated steam at a temperature of 155 degrees Celsius. Steel's coefficient of linear expansion is 1.2 X 10^-5 k-1. The pipe is allowed to expand freely when the steam is transported. What is the increase in the length of the pipe when it is used with the super heated steam?
60 mm
A camper is about to drink his morning coffee. He pours 400 grams of coffee, initially at 75°C into a 250-g aluminum cup, initially at 16°C. What is the equilibrium temperature of the coffee-cup system, assuming no heat is lost to the surroundings? The specific heat of aluminum is 900 J/kg • K, and the specific heat of coffee is essentially the same as that of water, which is 4186 J/kg • K.
68°C
It is necessary to determine the specific heat of an unknown object. The mass of the object is It is determined experimentally that it takes to raise the temperature What is the specific heat of the object?
7.46 J/kg • K
A gas expands from an initial volume of 0.040 m3 to a final volume of 0.085 m3 while its pressure increases linearly with the volume (so that the process follows a straight-line path in a pV diagram) from 110 kPa to 225 kPa. How much work is done by the gas during this expansion?
7.5 kJ
A container of 114.0 g of water is heated using 67 W of power, with perfect efficiency. How long will it take to raise the temperature of the water from 15 degrees Celsius to 25 degrees Celsius The specific heat capacity of the container is negligible, and the specific heat capacity of water is 4.186 ¥ 103 J/kg • C.
71 s
In a flask, 114.0 g of water is heated using of power, with perfect efficiency. How long will it take to raise the temperature of the water from to The specific heat of water is 4186 J/kg • K.
71 s
How much heat must be added to a 8.0-kg block of ice at -8°C to change it to water at The specific heat of ice is 2050 J/kg • C°.
780 kcal
A certain gas is compressed adiabatically. The amount of work done on the gas is 800 J. What is the change in the internal (thermal) energy of the gas?
800 J
A 6.5-g iron meteor hits the earth at a speed of 295 m/s. If its kinetic energy is entirely converted to heat in the meteor, by how much will its temperature rise? The specific heat of iron is 113 cal/kg • C°, and 1 cal = 4.186 J.
92.0 C°
A 2294-kg sample of water at 0° C is cooled to and freezes in the process. How much heat is -36 degrees Celsius liberated? The specific heat of ice is 2050 J/kg • K.
935,000 kJ
At what point on the figure above does the substance undergo a phase change?
B
How is conservation of internal energy expressed for a system during an isothermal process?
DT = 0, so DU = 0; therefore, DU = Q - W = 0, or Q = W
In an elastic collision between two ball bearings, kinetic energy is conserved. If there is no change in potential energy, which of the following is true?
DU = 0
How is conservation of internal energy expressed for a system during an isometrically process?
DV = 0, so PDV = 0 and W = 0; therefore, DU = Q
What accounts for an increase in the temperature of a gas that is kept at constant volume?
Energy has been added as heat to the gas.
If there is no temperature difference between a substance and its surroundings, what has occurred on the microscopic level?
Energy has been transferred from higher-energy particles to lower-energy particles.
Why does sandpaper get hot when it is rubbed against rusty metal?
Friction between the sandpaper and metal increases the temperature of both.
A nail is driven into a board with an initial kinetic energy of 150 J. If the potential energy before and after the event is the same, what is the change in the internal energy of the board and nail?
Given: KEi = 150 J KE f = 0 J DPE = 0 J Solution: The nail comes to rest in the board, so the final kinetic energy equals zero. Thus the change in kinetic energy is 150 J. From the conservation of energy, DPE + DKE + DU = 0 0 + KE f - KEi + DU = 0 DU = KEi = 150 J
A slice of bread contains about 4.19 X 105 J of energy. If the specific heat capacity of a person is 4.19 X 103 J/kg·°C, by how many degrees Celsius would the temperature of a 70.0 kg person increase if all the energy in the bread were converted to heat?
Given: Qbread = 4.19 X 105 J c p,person = 4.19 X 103 J/kg·°C mperson = 70.0 kg Solution: Qbread = c p,personmpersonDTperson DTperson = Qbread c p,personmperson = 4.19 X 105 J (4.19 X 103 J/kg°C)(70.0 kg) = 1.43°C
According to the second law of thermodynamics, which of the following statements about a heat engine operating in a complete cycle must be true?
Heat from a high-temperature reservoir cannot be completely converted to work.
Which of the following would you wear outside if it were 70 degrees celcius?
It cannot get that hot outside on Earth.
The coefficient of linear expansion of copper is 17 ¥ 10-6 K-1. A sheet of copper has a round hole with a radius of 3.0 m cut out of it. If the sheet is heated and undergoes a change in temperature of 80 K, what is the change in the radius of the hole?
It increases by 4.1 mm.
A thermodynamic process occurs, and the entropy of a system decreases. What can be concluded about the entropy change of the environment?
It increases.
What happens to the internal energy of an ideal gas when it is heated from 0°C to 4°C?
It increases.
A thermally isolated system is made up of a hot piece of aluminum and a cold piece of copper, with the aluminum and the copper in thermal contact. The specific heat capacity of aluminum is more than double that of copper. Which object experiences the greater temperature change during the time the system takes to reach thermal equilibrium?
It is impossible to tell without knowing the masses.
A heat engine has taken in energy as heat and used a portion of it to do work. What must happen next for the engine to complete the cycle and return to its initial conditions?
It must give up energy as heat to a lower temperature so work can be done on it.
A chunk of ice with a mass of 1 kg at 0°C melts and absorbs 3.33 ¥ 105 J of heat in the process. Which best describes what happened to this system?
Its entropy increased.
Imagine you could observe the individual atoms that make up a piece of matter and that you observe the motion of the atoms becoming more orderly. What can you assume about the system?
Its entropy is decreasing.
Which of the following is not a widely used temperature scale?
Joule
Which of the following is a direct cause of a substance's temperature increase?
Kinetic energy is added to the particles of the substance.
What occurs when a system's disorder is increased?
Less energy is available to do work.
A thermally isolated system is made up of a hot piece of aluminum and a cold piece of copper, with the aluminum and the copper in thermal contact. The specific heat capacity of aluminum is more than double that of copper. Which object experiences the greater magnitude gain or loss of heat during the time the system takes to reach thermal equilibrium?
Neither one; both of them experience the same size gain or loss of heat.
Which of the following best describes the relationship between two systems in thermal equilibrium?
No net energy is exchanged.
How is conservation of internal energy expressed for a system during an adiabatic process?
Q = 0, so DU = -W
How is conservation of internal energy expressed for an isolated system?
Q = W = 0, so DU = 0 and Ui = U f
Which of the following is true during a phase change?
Temperature remains constant.
Energy transfer as heat between two objects depends on which of the following?
The difference in temperature of the two objects.
If two small beakers of water, one at 70°C and one at 80°C, are emptied into a large beaker, what is the final temperature of the water?
The final temperature is between 70°C and 80°C.
If energy is transferred from a table to a block of ice moving across the table, which of the following statements is true?
The ice is cooler than the table.
Which statement applies when all of the entropy changes in a process are taken into account?
The increases in entropy are always greater than the decreases.
In the presence of friction, not all of the work done on a system appears as mechanical energy. What happens to the rest of the energy provided by work?
The remaining energy causes an increase in the internal energy of the system.
When a drop of ink mixes with water, what happens to the entropy of the system?
The system's entropy increases, and the total entropy of the universe increases.
Which of the following is not a way in which a cyclic process resembles an isothermal process?
The temperature of the system remains constant throughout the process.
The figure above shows how the temperature of 10.0 g of ice changes as energy is added. Which of the following statements is correct?
The water absorbed energy continuously, but the temperature increased only when all of the water was in one phase.
Which equation describes the net work done for a complete cycle of a heat engine?
Wnet = Qh - Qc
Which of the following is a thermodynamic process in which a system returns to the same conditions under which it started?
a cyclic process
Which of the following would you wear outside if it were 20 degrees Celcius?
a short sleeve shirt, but long warm pants
Which of the following is a set of particles or interacting components to which energy is added or from which energy is removed?
a system
Air cools as it escapes from a diver's compressed air tank. What kind of process is this?
adiabatic
Which thermodynamic process takes place when work is done on or by the system but no energy is transferred to or from the system as heat?
adiabatic
The use of fiberglass insulation in the outer walls of a building is intended to minimize heat transfer through what process?
conduction
The process in which heat flows by the mass movement of molecules from one place to another is known as
convection.
Which of the following is a good conductor of heat?
copper
As shown in the figure, a bimetallic strip, consisting of metal G on the top and metal H on the bottom, is rigidly attached to a wall at the left. The coefficient of linear thermal expansion for metal G is greater than that of metal H. If the strip is uniformly heated, it will
curve downward.
When water at 0°C freezes, the entropy of the water
decreases.
The second law of thermodynamics leads us to conclude that
disorder in the universe is increasing with the passage of time.
To which of the following is high temperature related?
high particle kinetic energy
Which of the following is a way to improve the efficiency of a heat engine?
increase Qh
An ideal gas undergoes an isothermal expansion. During this process, its entropy
increases.
In an isovolumetric process for an ideal gas, the system's change in the energy as heat is equivalent to a change in which of the following?
internal energy
What are the energies associated with atomic motion called?
internal energy
According to the first law of thermodynamics, the difference between energy transferred to or from a system as heat and energy transferred to or from a system by work is equivalent to which of the following?
internal energy change
A cyclic process is carried out on an ideal gas such that it returns to its initial state at the end of a cycle, as shown in the pV diagram in the figure. If the process is carried out in a clockwise sense around the enclosed area, as shown on the figure, then the change of internal energy over the full cycle
is zero.
What three properties of a substance affect the amount of energy transferred as heat to or from the substance?
mass, temperature change, specific heat capacity
A calorimeter is used to determine the specific heat capacity of a test metal. If the specific heat capacity of water is known, what quantities must be measured?
metal mass, water mass, initial and final temperatures of metal and water
The requirement that a heat engine must give up some energy at a lower temperature in order to do work corresponds to which law of thermodynamics?
second
Which of the following would you wear outside if it were 40 degrees Celcius?
shorts and a tank top
If you wanted to know how much the temperature of a particular piece of material would rise when a known amount of heat was added to it, which of the following quantities would be most helpful to know?
specific heat
Which of the following describes a substance in which the temperature and pressure remain constant while the substance experiences an inward transfer of energy?
substance undergoing a change of state
When a gas expands adiabatically,
the internal (thermal) energy of the gas decreases.
A cyclic process is carried out on an ideal gas such that it returns to its initial state at the end of a cycle, as shown in the pV diagram in the figure. If the process is carried out in a clockwise sense around the enclosed area, as shown on the figure, then the magnitude of the enclosed area represents
the work done by the gas.
A cyclic process is carried out on an ideal gas such that it returns to its initial state at the end of a cycle, as shown in the pV diagram in the figure. If the process is carried out in a counter-clockwise sense around the enclosed area, as shown on the figure, then the magnitude of the enclosed area represents
the work done on the gas.
On a cold day, a piece of metal feels much colder to the touch than a piece of wood. This is due to the difference in which one of the following physical properties of these materials?
thermal conductivity
As the temperature of a substance increases, its volume tends to increase due to
thermal expansion.
During an isometrically process, which of the following does not change?
volume
When an ideal gas does positive work on its surroundings, which of the gas's quantities increases?
volume
