Podcast
Questions and Answers
For an isobaric process, which of the following statements correctly describes the relationship between work (W), pressure (p), and volume change (V₂ - V₁)?
For an isobaric process, which of the following statements correctly describes the relationship between work (W), pressure (p), and volume change (V₂ - V₁)?
- W = V₂ - V₁
- W = p / (V₂ - V₁)
- W = pV₁V₂
- W = p(V₂ - V₁) (correct)
During an adiabatic process, what condition holds true regarding heat transfer (Q) between the system and its surroundings?
During an adiabatic process, what condition holds true regarding heat transfer (Q) between the system and its surroundings?
- Q is infinite, indicating instantaneous heat transfer.
- Q < 0, indicating heat is removed from the system.
- Q = 0, indicating no heat transfer. (correct)
- Q > 0, indicating heat is added to the system.
A thermodynamic system undergoes a process where its internal energy remains constant. Which of the following statements must be true about this process?
A thermodynamic system undergoes a process where its internal energy remains constant. Which of the following statements must be true about this process?
- The work done by the system is greater than the heat added to it.
- The system performs work equal to the heat added to it. (correct)
- No work is done by or on the system.
- The heat added to the system is zero.
For an ideal gas, under what condition does the internal energy depend only on its temperature?
For an ideal gas, under what condition does the internal energy depend only on its temperature?
Which type of thermodynamic process is characterized by a constant volume?
Which type of thermodynamic process is characterized by a constant volume?
If a system absorbs 150 J of heat and performs 100 J of work, what is the change in internal energy of the system?
If a system absorbs 150 J of heat and performs 100 J of work, what is the change in internal energy of the system?
In adiabatic processes involving ideal gases, which of the following quantities remains constant?
In adiabatic processes involving ideal gases, which of the following quantities remains constant?
What does a negative value of work (W) indicate in a thermodynamic process?
What does a negative value of work (W) indicate in a thermodynamic process?
What is the relationship between molar heat capacities at constant pressure ($C_p$) and constant volume ($C_v$) for an ideal gas, in terms of the ideal gas constant (R)?
What is the relationship between molar heat capacities at constant pressure ($C_p$) and constant volume ($C_v$) for an ideal gas, in terms of the ideal gas constant (R)?
Consider a thermodynamic process. The heat added to the system and the work done by the system depend on:
Consider a thermodynamic process. The heat added to the system and the work done by the system depend on:
Flashcards
Thermodynamic Processes
Thermodynamic Processes
A thermodynamic system's potential to exchange energy with its surroundings.
1st Law of Thermodynamics
1st Law of Thermodynamics
The heat added equals the change in internal energy plus work done.
Adiabatic Process
Adiabatic Process
No heat exchange occurs.
Isochoric Process
Isochoric Process
Signup and view all the flashcards
Isobaric Process
Isobaric Process
Signup and view all the flashcards
Isothermal Process
Isothermal Process
Signup and view all the flashcards
Ideal Gas Internal Energy
Ideal Gas Internal Energy
Signup and view all the flashcards
Adiabatic ideal gas process
Adiabatic ideal gas process
Signup and view all the flashcards
Work in Thermodynamics
Work in Thermodynamics
Signup and view all the flashcards
Internal Energy (U)
Internal Energy (U)
Signup and view all the flashcards
Study Notes
Heat and Work in Thermodynamic Processes
- A thermodynamic system can exchange energy with its surroundings through heat transfer or mechanical work.
- When a system's volume changes from V₁ to V₂ at pressure p, the work W is the integral of p with respect to volume: W = ∫(from V₁ to V₂) pdV.
- For constant pressure, work done equals pressure times the change in volume: W = p(V₂ - V₁).
- A negative W indicates work done on the system.
- Heat added to the system and work done depend on the initial and final states and the path of intermediate states.
First Law of Thermodynamics
- The first law states that when heat Q is added to a system, and the system does work W, internal energy U changes by Q - W: ΔU = Q - W.
- This also applies to infinitesimal processes: dU = dQ - dW.
- Internal energy depends only on the system's state and the change in internal energy in a process depends on initial and final states, not the path.
- The internal energy of an isolated system remains constant.
Important Kinds of Thermodynamic Processes
- Adiabatic: No heat transfer (Q = 0).
- Isochoric: Constant volume, no work done (W = 0).
- Isobaric: Constant pressure, work done is W = p(V₂ - V₁).
- Isothermal: Constant temperature.
Thermodynamics of Ideal Gases
- Internal energy depends only on temperature, not pressure or volume.
- For other substances, internal energy depends on both pressure and temperature.
- Molar heat capacities Cₚ and Cᵥ of an ideal gas differ by R (ideal-gas constant): Cₚ = Cᵥ + R.
- The dimensionless ratio of heat capacities, Cₚ/Cᵥ, is denoted by γ: γ = Cₚ/Cᵥ.
Adiabatic Processes in Ideal Gases
- For an adiabatic process with an ideal gas, TV^(γ-1) and pV^γ are constant.
- Work done by an ideal gas during adiabatic expansion can be expressed in terms of initial and final temperatures: W = nCᵥ(T₁ - T₂).
- Work can also be expressed with initial and final values of pressure and volume: W = (Cᵥ/R)(p₁V₁ - p₂V₂) = (1/(γ-1))(p₁V₁ - p₂V₂).
Studying That Suits You
Use AI to generate personalized quizzes and flashcards to suit your learning preferences.
