B.4 Thermodynamics

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Directly related questions

EXE.1A.HL.TZ0.23: Three statements about the Carnot cycle are: I. The Carnot cycle is reversible.II. The net...
EXE.1A.HL.TZ0.23: Three statements about the Carnot cycle are: I. The Carnot cycle is reversible.II. The net...
EXE.1A.HL.TZ0.17: A thermodynamic cycle consisting of an adiabatic, isovolumetric and isothermal processes is...
EXE.1A.HL.TZ0.17: A thermodynamic cycle consisting of an adiabatic, isovolumetric and isothermal processes is...
EXE.1A.HL.TZ0.18: An ideal gas expands isothermally. The work done by the gas is 100 J. What is the change in the...
EXE.1A.HL.TZ0.18: An ideal gas expands isothermally. The work done by the gas is 100 J. What is the change in the...
EXE.1A.HL.TZ0.19: A thermodynamic process taking place in an isolated system is irreversible when the final state...
EXE.1A.HL.TZ0.19: A thermodynamic process taking place in an isolated system is irreversible when the final state...
EXE.1A.HL.TZ0.20: Which statement is correct about the entropy of a non-isolated system? A. It always...
EXE.1A.HL.TZ0.20: Which statement is correct about the entropy of a non-isolated system? A. It always...
EXE.1A.HL.TZ0.21: An energy of 200 J is transferred isothermally to an ideal gas. The temperature of the gas is...
EXE.1A.HL.TZ0.21: An energy of 200 J is transferred isothermally to an ideal gas. The temperature of the gas is...
EXE.1A.HL.TZ0.24: For a thermodynamic process, the entropy of the universe A. always increases during the...
EXE.1A.HL.TZ0.24: For a thermodynamic process, the entropy of the universe A. always increases during the...
EXE.1A.HL.TZ0.22: Energy is transferred very slowly to ice of mass 0.050 kg at its melting point so that the ice...
EXE.1A.HL.TZ0.22: Energy is transferred very slowly to ice of mass 0.050 kg at its melting point so that the ice...
EXE.2.HL.TZ0.1civ:
Determine the efficiency of the cycle.
EXE.2.HL.TZ0.1civ:
Determine the efficiency of the cycle.
EXE.2.HL.TZ0.iv:
Determine the efficiency of the cycle.
EXE.2.HL.TZ0.1ciii:
Outline why the entropy of the gas remains constant during changes BC and DA.
EXE.2.HL.TZ0.1ciii:
Outline why the entropy of the gas remains constant during changes BC and DA.
EXE.2.HL.TZ0.iii:
Outline why the entropy of the gas remains constant during changes BC and DA.
EXE.2.HL.TZ0.12a: State what is meant by an isolated system.
EXE.2.HL.TZ0.12a: State what is meant by an isolated system.
EXE.2.HL.TZ0.a: State what is meant by an isolated system.
EXE.2.HL.TZ0.14b:
A throw is made once every minute. Estimate the average time required before a throw occurs where all coins are heads or all coins are tails.
EXE.2.HL.TZ0.14b:
A throw is made once every minute. Estimate the average time required before a throw occurs where all coins are heads or all coins are tails.
EXE.2.HL.TZ0.b:
A throw is made once every minute. Estimate the average time required before a throw occurs where all coins are heads or all coins are tails.
EXE.2.HL.TZ0.12c:
Configuration B has 120 microstates. Calculate the entropy difference between configurations B and A. State the answer in terms of $k_{B}$ .
EXE.2.HL.TZ0.12c:
Configuration B has 120 microstates. Calculate the entropy difference between configurations B and A. State the answer in terms of $k_{B}$ .
EXE.2.HL.TZ0.c:
Configuration B has 120 microstates. Calculate the entropy difference between configurations B and A. State the answer in terms of $k_{B}$ .
EXE.2.HL.TZ0.14c:
In one throw the coins all land heads upwards. The following throw results in 7 heads and 3 tails. Calculate, in terms of $k_{B}$ , the change in entropy between the two throws.
EXE.2.HL.TZ0.14c:
In one throw the coins all land heads upwards. The following throw results in 7 heads and 3 tails. Calculate, in terms of $k_{B}$ , the change in entropy between the two throws.
EXE.2.HL.TZ0.c:
In one throw the coins all land heads upwards. The following throw results in 7 heads and 3 tails. Calculate, in terms of $k_{B}$ , the change in entropy between the two throws.
EXE.2.HL.TZ0.12b: State and explain the number of microstates of the system in configuration A.
EXE.2.HL.TZ0.12b: State and explain the number of microstates of the system in configuration A.
EXE.2.HL.TZ0.b: State and explain the number of microstates of the system in configuration A.
EXE.2.HL.TZ0.11a: Explain why the gas in configuration B has a greater number of microstates than in A.
EXE.2.HL.TZ0.11a: Explain why the gas in configuration B has a greater number of microstates than in A.
EXE.2.HL.TZ0.a: Explain why the gas in configuration B has a greater number of microstates than in A.
EXE.2.HL.TZ0.11b:
Deduce, with reference to entropy, that the expansion of the gas from the initial configuration A is irreversible.
EXE.2.HL.TZ0.11b:
Deduce, with reference to entropy, that the expansion of the gas from the initial configuration A is irreversible.
EXE.2.HL.TZ0.b:
Deduce, with reference to entropy, that the expansion of the gas from the initial configuration A is irreversible.
EXE.2.HL.TZ0.12d:
The system is initially in configuration A. Comment, with reference to the second law of thermodynamics and your answer in (c), on the likely evolution of the system.
EXE.2.HL.TZ0.12d:
The system is initially in configuration A. Comment, with reference to the second law of thermodynamics and your answer in (c), on the likely evolution of the system.
EXE.2.HL.TZ0.d:
The system is initially in configuration A. Comment, with reference to the second law of thermodynamics and your answer in (c), on the likely evolution of the system.
EXE.2.HL.TZ0.13a:
Outline, using these two cases as examples, the distinction between a microstate and a macrostate.
EXE.2.HL.TZ0.a:
Outline, using these two cases as examples, the distinction between a microstate and a macrostate.
EXE.2.HL.TZ0.14a: Determine the fractional number of throws for which the three most likely macrostates occur.
EXE.2.HL.TZ0.14a: Determine the fractional number of throws for which the three most likely macrostates occur.
EXE.2.HL.TZ0.a: Determine the fractional number of throws for which the three most likely macrostates occur.
23M.2.SL.TZ1.7d:
Calculate the thermal energy (heat) taken out of the gas from B to C.
23M.2.SL.TZ1.9d:
Calculate the thermal energy (heat) taken out of the gas from B to C.
23M.2.SL.TZ1.d:
Calculate the thermal energy (heat) taken out of the gas from B to C.
23M.2.SL.TZ1.d:
Calculate the thermal energy (heat) taken out of the gas from B to C.
23M.2.SL.TZ1.9a: Suggest why AC is the adiabatic part of the cycle.
23M.2.SL.TZ1.7a: Suggest why AC is the adiabatic part of the cycle.
23M.2.SL.TZ1.a: Suggest why AC is the adiabatic part of the cycle.
23M.2.SL.TZ1.a: Suggest why AC is the adiabatic part of the cycle.
23M.2.SL.TZ1.9c:
Suggest, for the change A ⇒ B, whether the entropy of the gas is increasing, decreasing or constant.
23M.2.SL.TZ1.7c:
Suggest, for the change A ⇒ B, whether the entropy of the gas is increasing, decreasing or constant.
23M.2.SL.TZ1.c:
Suggest, for the change A ⇒ B, whether the entropy of the gas is increasing, decreasing or constant.
23M.2.SL.TZ1.c:
Suggest, for the change A ⇒ B, whether the entropy of the gas is increasing, decreasing or constant.
23M.2.SL.TZ1.9e:
The highest and lowest temperatures of the gas during the cycle are 602 K and 92 K.

The efficiency of this engine is about 0.6. Outline how these data are consistent with the second law of thermodynamics.
23M.2.SL.TZ1.7e:
The highest and lowest temperatures of the gas during the cycle are 602 K and 92 K.

The efficiency of this engine is about 0.6. Outline how these data are consistent with the second law of thermodynamics.
23M.2.SL.TZ1.e:
The highest and lowest temperatures of the gas during the cycle are 602 K and 92 K.

The efficiency of this engine is about 0.6. Outline how these data are consistent with the second law of thermodynamics.
23M.2.SL.TZ1.e:
The highest and lowest temperatures of the gas during the cycle are 602 K and 92 K.

The efficiency of this engine is about 0.6. Outline how these data are consistent with the second law of thermodynamics.
23M.2.SL.TZ1.9b:
Show that the volume at C is 3.33 × 10⁻² m³.
23M.2.SL.TZ1.7b:
Show that the volume at C is 3.33 × 10⁻² m³.
23M.2.SL.TZ1.b:
Show that the volume at C is 3.33 × 10⁻² m³.
23M.2.SL.TZ1.b:
Show that the volume at C is 3.33 × 10⁻² m³.
23M.2.HL.TZ2.9e:
Explain why the work done by the gas during the isothermal expansion AB is less than the work done on the gas during the adiabatic compression BC.
23M.2.HL.TZ2.7e:
Explain why the work done by the gas during the isothermal expansion AB is less than the work done on the gas during the adiabatic compression BC.
23M.2.HL.TZ2.e:
Explain why the work done by the gas during the isothermal expansion AB is less than the work done on the gas during the adiabatic compression BC.
23M.2.HL.TZ2.e:
Explain why the work done by the gas during the isothermal expansion AB is less than the work done on the gas during the adiabatic compression BC.
23M.2.HL.TZ2.9a:
Calculate the pressure of the gas at B.
23M.2.HL.TZ2.7a:
Calculate the pressure of the gas at B.
23M.2.HL.TZ2.a:
Calculate the pressure of the gas at B.
23M.2.HL.TZ2.a:
Calculate the pressure of the gas at B.
23M.2.HL.TZ2.9d: Explain why the change of entropy for the gas during the process BC is equal to zero.
23M.2.HL.TZ2.7d: Explain why the change of entropy for the gas during the process BC is equal to zero.
23M.2.HL.TZ2.d: Explain why the change of entropy for the gas during the process BC is equal to zero.
23M.2.HL.TZ2.d: Explain why the change of entropy for the gas during the process BC is equal to zero.
23M.2.HL.TZ2.7b:
Sketch, on the pV diagram, the remaining two processes BC and CA that the gas undergoes.
23M.2.HL.TZ2.9b:
Sketch, on the pV diagram, the remaining two processes BC and CA that the gas undergoes.
23M.2.HL.TZ2.b:
Sketch, on the pV diagram, the remaining two processes BC and CA that the gas undergoes.
23M.2.HL.TZ2.b:
Sketch, on the pV diagram, the remaining two processes BC and CA that the gas undergoes.
23M.2.HL.TZ2.9c:
Show that the temperature of the gas at C is approximately 350 °C.
23M.2.HL.TZ2.7c:
Show that the temperature of the gas at C is approximately 350 °C.
23M.2.HL.TZ2.c:
Show that the temperature of the gas at C is approximately 350 °C.
23M.2.HL.TZ2.c:
Show that the temperature of the gas at C is approximately 350 °C.
23M.2.HL.TZ2.7f:
The quantity of trapped gas is 53.2 mol. Calculate the thermal energy removed from the gas during process CA.
23M.2.HL.TZ2.9f:
The quantity of trapped gas is 53.2 mol. Calculate the thermal energy removed from the gas during process CA.
23M.2.HL.TZ2.f:
The quantity of trapped gas is 53.2 mol. Calculate the thermal energy removed from the gas during process CA.
23M.2.HL.TZ2.f:
The quantity of trapped gas is 53.2 mol. Calculate the thermal energy removed from the gas during process CA.
SPM.1A.HL.TZ0.11: A gas undergoes one cycle of a cyclic process. The net change in internal energy of the gas...
SPM.1A.HL.TZ0.11: A gas undergoes one cycle of a cyclic process. The net change in internal energy of the gas...
SPM.1A.HL.TZ0.11: A gas undergoes one cycle of a cyclic process. The net change in internal energy of the gas...
SPM.1A.HL.TZ0.11: A gas undergoes one cycle of a cyclic process. The net change in internal energy of the gas...
SPM.1A.HL.TZ0.12: A working refrigerator with the door open is placed in a sealed room. The entropy of the room A. ...
SPM.1A.HL.TZ0.12: A working refrigerator with the door open is placed in a sealed room. The entropy of the room A. ...
SPM.1A.HL.TZ0.12: A working refrigerator with the door open is placed in a sealed room. The entropy of the room A. ...
SPM.1A.HL.TZ0.12: A working refrigerator with the door open is placed in a sealed room. The entropy of the room A. ...
19M.2.HL.TZ1.7a:
Show that during an adiabatic expansion of an ideal monatomic gas the temperature $T$ and volume $V$ are given by

$T{V^{\frac{2}{3}}}$ = constant
19M.2.HL.TZ1.a:
Show that during an adiabatic expansion of an ideal monatomic gas the temperature $T$ and volume $V$ are given by

$T{V^{\frac{2}{3}}}$ = constant
19M.2.HL.TZ1.7b.i:
Calculate the efficiency of the cycle.
19M.2.HL.TZ1.b.i:
Calculate the efficiency of the cycle.
19M.2.HL.TZ1.7b.ii:
The work done during the isothermal expansion A → B is 540 J. Calculate the thermal energy that leaves the gas during one cycle.
19M.2.HL.TZ1.b.ii:
The work done during the isothermal expansion A → B is 540 J. Calculate the thermal energy that leaves the gas during one cycle.
19M.2.HL.TZ1.7b.iii:
Calculate the ratio $\frac{{{V_C}}}{{{V_B}}}$ where V_C is the volume of the gas at C and V_B is the volume at B.
19M.2.HL.TZ1.b.iii:
Calculate the ratio $\frac{{{V_C}}}{{{V_B}}}$ where V_C is the volume of the gas at C and V_B is the volume at B.
19M.2.HL.TZ1.7c.i:
Calculate the change in the entropy of the gas during the change A to B.
19M.2.HL.TZ1.c.i:
Calculate the change in the entropy of the gas during the change A to B.
19M.2.HL.TZ1.7c.ii:
Explain, by reference to the second law of thermodynamics, why a real engine operating between the temperatures of 620 K and 340 K cannot have an efficiency greater than the answer to (b)(i).
19M.2.HL.TZ1.c.ii:
Explain, by reference to the second law of thermodynamics, why a real engine operating between the temperatures of 620 K and 340 K cannot have an efficiency greater than the answer to (b)(i).
19M.2.HL.TZ2.10a:
Show that the work done on the gas for the isothermal process C→A is approximately 440 J.
19M.2.HL.TZ2.a:
Show that the work done on the gas for the isothermal process C→A is approximately 440 J.
19M.2.HL.TZ2.10bi:
Calculate the change in internal energy of the gas for the process A→B.
19M.2.HL.TZ2.bi:
Calculate the change in internal energy of the gas for the process A→B.
19M.2.HL.TZ2.10bii: Calculate the temperature at A if the temperature at B is −40°C.
19M.2.HL.TZ2.bii: Calculate the temperature at A if the temperature at B is −40°C.
19M.2.HL.TZ2.10c: Determine, using the first law of thermodynamics, the total thermal energy transferred to the...
19M.2.HL.TZ2.c: Determine, using the first law of thermodynamics, the total thermal energy transferred to the...
19M.2.HL.TZ2.10d: Suggest why this cycle is not a suitable model for a working heat pump.
19M.2.HL.TZ2.d: Suggest why this cycle is not a suitable model for a working heat pump.
20N.2.HL.TZ0.9a(i):
Calculate the work done during the compression.
20N.2.HL.TZ0.a(i):
Calculate the work done during the compression.
20N.2.HL.TZ0.9a(ii):
Calculate the work done during the increase in pressure.
20N.2.HL.TZ0.a(ii):
Calculate the work done during the increase in pressure.
20N.2.HL.TZ0.9b(i):
Calculate the pressure following this process.
20N.2.HL.TZ0.b(i):
Calculate the pressure following this process.
20N.2.HL.TZ0.9b(ii): Outline how an approximate adiabatic change can be achieved.
20N.2.HL.TZ0.b(ii): Outline how an approximate adiabatic change can be achieved.
23M.2.SL.TZ1.9a: Suggest why AC is the adiabatic part of the cycle.
23M.2.SL.TZ1.7a: Suggest why AC is the adiabatic part of the cycle.
23M.2.SL.TZ1.a: Suggest why AC is the adiabatic part of the cycle.
23M.2.SL.TZ1.a: Suggest why AC is the adiabatic part of the cycle.
23M.2.SL.TZ1.9b:
Show that the volume at C is 3.33 × 10⁻² m³.
23M.2.SL.TZ1.7b:
Show that the volume at C is 3.33 × 10⁻² m³.
23M.2.SL.TZ1.b:
Show that the volume at C is 3.33 × 10⁻² m³.
23M.2.SL.TZ1.b:
Show that the volume at C is 3.33 × 10⁻² m³.
23M.2.SL.TZ1.9c:
Suggest, for the change A ⇒ B, whether the entropy of the gas is increasing, decreasing or constant.
23M.2.SL.TZ1.7c:
Suggest, for the change A ⇒ B, whether the entropy of the gas is increasing, decreasing or constant.
23M.2.SL.TZ1.c:
Suggest, for the change A ⇒ B, whether the entropy of the gas is increasing, decreasing or constant.
23M.2.SL.TZ1.c:
Suggest, for the change A ⇒ B, whether the entropy of the gas is increasing, decreasing or constant.
23M.2.SL.TZ1.7d:
Calculate the thermal energy (heat) taken out of the gas from B to C.
23M.2.SL.TZ1.9d:
Calculate the thermal energy (heat) taken out of the gas from B to C.
23M.2.SL.TZ1.d:
Calculate the thermal energy (heat) taken out of the gas from B to C.
23M.2.SL.TZ1.d:
Calculate the thermal energy (heat) taken out of the gas from B to C.
23M.2.SL.TZ1.9e:
The highest and lowest temperatures of the gas during the cycle are 602 K and 92 K.

The efficiency of this engine is about 0.6. Outline how these data are consistent with the second law of thermodynamics.
23M.2.SL.TZ1.7e:
The highest and lowest temperatures of the gas during the cycle are 602 K and 92 K.

The efficiency of this engine is about 0.6. Outline how these data are consistent with the second law of thermodynamics.
23M.2.SL.TZ1.e:
The highest and lowest temperatures of the gas during the cycle are 602 K and 92 K.

The efficiency of this engine is about 0.6. Outline how these data are consistent with the second law of thermodynamics.
23M.2.SL.TZ1.e:
The highest and lowest temperatures of the gas during the cycle are 602 K and 92 K.

The efficiency of this engine is about 0.6. Outline how these data are consistent with the second law of thermodynamics.
23M.2.HL.TZ2.9a:
Calculate the pressure of the gas at B.
23M.2.HL.TZ2.7a:
Calculate the pressure of the gas at B.
23M.2.HL.TZ2.a:
Calculate the pressure of the gas at B.
23M.2.HL.TZ2.a:
Calculate the pressure of the gas at B.
23M.2.HL.TZ2.7b:
Sketch, on the pV diagram, the remaining two processes BC and CA that the gas undergoes.
23M.2.HL.TZ2.9b:
Sketch, on the pV diagram, the remaining two processes BC and CA that the gas undergoes.
23M.2.HL.TZ2.b:
Sketch, on the pV diagram, the remaining two processes BC and CA that the gas undergoes.
23M.2.HL.TZ2.b:
Sketch, on the pV diagram, the remaining two processes BC and CA that the gas undergoes.
23M.2.HL.TZ2.9c:
Show that the temperature of the gas at C is approximately 350 °C.
23M.2.HL.TZ2.7c:
Show that the temperature of the gas at C is approximately 350 °C.
23M.2.HL.TZ2.c:
Show that the temperature of the gas at C is approximately 350 °C.
23M.2.HL.TZ2.c:
Show that the temperature of the gas at C is approximately 350 °C.
23M.2.HL.TZ2.9d: Explain why the change of entropy for the gas during the process BC is equal to zero.
23M.2.HL.TZ2.7d: Explain why the change of entropy for the gas during the process BC is equal to zero.
23M.2.HL.TZ2.d: Explain why the change of entropy for the gas during the process BC is equal to zero.
23M.2.HL.TZ2.d: Explain why the change of entropy for the gas during the process BC is equal to zero.
23M.2.HL.TZ2.9e:
Explain why the work done by the gas during the isothermal expansion AB is less than the work done on the gas during the adiabatic compression BC.
23M.2.HL.TZ2.7e:
Explain why the work done by the gas during the isothermal expansion AB is less than the work done on the gas during the adiabatic compression BC.
23M.2.HL.TZ2.e:
Explain why the work done by the gas during the isothermal expansion AB is less than the work done on the gas during the adiabatic compression BC.
23M.2.HL.TZ2.e:
Explain why the work done by the gas during the isothermal expansion AB is less than the work done on the gas during the adiabatic compression BC.
23M.2.HL.TZ2.7f:
The quantity of trapped gas is 53.2 mol. Calculate the thermal energy removed from the gas during process CA.
23M.2.HL.TZ2.9f:
The quantity of trapped gas is 53.2 mol. Calculate the thermal energy removed from the gas during process CA.
23M.2.HL.TZ2.f:
The quantity of trapped gas is 53.2 mol. Calculate the thermal energy removed from the gas during process CA.
23M.2.HL.TZ2.f:
The quantity of trapped gas is 53.2 mol. Calculate the thermal energy removed from the gas during process CA.

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B.4 Thermodynamics

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