Laws of Thermodynamics Quiz
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Laws of Thermodynamics Quiz

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What does the first law of thermodynamics state?

  • The temperature of an isolated system approaches absolute zero.
  • The entropy of an isolated system always decreases.
  • Energy can be created or destroyed in an isolated system.
  • Energy cannot be created or destroyed in an isolated system. (correct)

    • According to the second law of thermodynamics, what happens to the entropy of an isolated system?

  • It becomes zero at absolute zero.
  • It decreases over time.
  • It always increases. (correct)
  • It remains constant.

    • What occurs during an isobaric process?

  • No heat is absorbed or released.
  • Temperature remains constant.
  • Volume remains constant.
  • Pressure remains constant. (correct)

    • What characterizes a spontaneous process?

    <p>It occurs without being driven by an energy source.</p> Signup and view all the answers

    What does the third law of thermodynamics state about entropy as it approaches absolute zero?

    <p>Entropy approaches a constant value.</p> Signup and view all the answers

    What is thermodynamic work?

    <p>It occurs when the volume changes under pressure.</p> Signup and view all the answers

    Which of the following describes an adiabatic process?

    <p>No heat is exchanged with the surroundings.</p> Signup and view all the answers

    In the context of heat capacity, what does it measure?

    <p>How much heat a substance absorbs to increase its temperature by a specified amount.</p> Signup and view all the answers

    What does the negative sign in the work done indicate?

    <p>Work is done on the gas.</p> Signup and view all the answers

    What is the expression for work done on a monoatomic ideal gas during isothermal compression?

    <p>$W = P_o V_o [ln(V) - ln(V_o)]$</p> Signup and view all the answers

    What remains constant for the internal energy of a monoatomic ideal gas in an isothermal process?

    <p>Temperature</p> Signup and view all the answers

    In the first law of thermodynamics, how can heat exchanged be calculated?

    <p>Q = ΔU + W</p> Signup and view all the answers

    What is the value of the change in internal energy for the gas in this process?

    <p>$0$</p> Signup and view all the answers

    What happens to the amount of heat exchanged when the gas is compressed?

    <p>It decreases.</p> Signup and view all the answers

    What does the term ln(4) imply in the context of this thermodynamic process?

    <p>It is part of the expression for work done.</p> Signup and view all the answers

    How can the work done on the gas be expressed numerically?

    <p>$-80 ln(4) kJ$</p> Signup and view all the answers

    In an isochoric process, what is the relationship between heat exchanged and internal energy change?

    <p>Internal energy change is equal to heat exchanged.</p> Signup and view all the answers

    What characterizes the area under a P-V diagram during an expansion process?

    <p>The area is positive.</p> Signup and view all the answers

    Which of the following describes an isobaric process?

    <p>Pressure remains constant and work done can be expressed as W = PΔV.</p> Signup and view all the answers

    For a free expansion process under zero pressure, what is the impact on work done?

    <p>No work is done on or by the system.</p> Signup and view all the answers

    In relation to internal energy, what does the first law of thermodynamics state for an isobaric process?

    <p>Internal energy change equals heat exchanged minus work done.</p> Signup and view all the answers

    What does the integration of pressure as a function of volume determine in thermal physics?

    <p>The work done by or on the system.</p> Signup and view all the answers

    What is the heat exchange expression for a process at constant volume?

    <p>dQ = nCV dT.</p> Signup and view all the answers

    Which thermodynamic process is represented by a horizontal line on a P-V diagram?

    <p>Isobaric process.</p> Signup and view all the answers

    What is the relationship between the specific heats at constant volume and constant pressure for an ideal gas?

    <p>$c_v = c_p - R$</p> Signup and view all the answers

    Which equation represents the first law of thermodynamics for an isochor?

    <p>$\Delta U = Q$</p> Signup and view all the answers

    What does the variable $W$ represent in the context of the first law of thermodynamics?

    <p>Work done by the system</p> Signup and view all the answers

    For an ideal gas, what happens to the pressure and volume during an adiabatic process?

    <p>Pressure increases and volume decreases</p> Signup and view all the answers

    What can be inferred about the internal energy change ($\Delta U$) of an ideal gas?

    <p>It depends on temperature changes</p> Signup and view all the answers

    What equation expresses the relationship between pressure, volume, and temperature for an ideal gas?

    <p>$PV = nRT$</p> Signup and view all the answers

    How is work ($W$) calculated during an isobaric process?

    <p>By finding $P \Delta V$</p> Signup and view all the answers

    What defines the adiabatic index ($\gamma$) for a monatomic ideal gas?

    <p>$\gamma = \frac{c_p}{c_v}$</p> Signup and view all the answers

    During an adiabatic process, how does the internal energy ($\Delta U$) change?

    <p>It is equal to work done on the system</p> Signup and view all the answers

    What is the value of the internal energy change ∆U_C_A?

    <p>-360 kJ</p> Signup and view all the answers

    What is the expression for the net work done in the cycle?

    <p>(80,000) ln(4) J - 240,000 J</p> Signup and view all the answers

    After calculating, what is the numerical value of the net work done during the cycle?

    <p>-129 kJ</p> Signup and view all the answers

    What is the principle that verifies that the internal energy change for a complete cycle is zero?

    <p>Internal energy is path-independent</p> Signup and view all the answers

    What is the calculated value of net heat charge Q_net for the complete cycle?

    <p>-129 kJ</p> Signup and view all the answers

    In an isothermal process for an ideal gas, what happens to the internal energy?

    <p>It remains constant</p> Signup and view all the answers

    According to the first law of thermodynamics, what relates the change in internal energy to heat and work?

    <p>∆U = Q - W</p> Signup and view all the answers

    What is the relationship between heat added and work done in an ideal isothermal process?

    <p>Heat added equals work done</p> Signup and view all the answers

    How is the change in entropy ∆S calculated during a reversible process?

    <p>∆S = ∫(dQ/T)</p> Signup and view all the answers

    If the net internal energy change is zero for a complete cycle, what other variables must also satisfy this condition?

    <p>Q_net = W_net and ∆U_net = 0</p> Signup and view all the answers

    Study Notes

    Laws of Thermodynamics

    • The First Law of Thermodynamics states that energy cannot be created or destroyed in an isolated system. This is also known as the Law of Conservation of Energy.
    • The Second Law of Thermodynamics establishes that the entropy of any isolated system always increases.
    • The Third Law of Thermodynamics states that the entropy of a system approaches a constant value as the temperature approaches absolute zero.

    Key Terms

    • Pressure is the force applied per unit area.
    • Volume is the amount of space an object occupies.
    • Temperature measures the average kinetic energy of the molecules in a substance.
    • Absolute Zero is the lowest theoretically possible temperature.
    • Entropy is a thermodynamic property that measures a system's thermal energy per unit of temperature that is unavailable for useful work.
    • Work is done when the volume changes under pressure.
    • Heat is the thermal energy transferred between substances.
    • Heat Capacity measures the amount of heat a substance needs to absorb to increase its temperature by a specific amount.
    • Internal Energy refers to the total energy of a substance's molecules, excluding interactions with external fields.
    • Isothermal processes maintain a constant temperature.
    • Isobaric processes maintain a constant pressure.
    • Isochoric processes maintain a constant volume.
    • Adiabatic processes do not permit any heat absorption or release.
    • Isentropic processes maintain a constant entropy.
    • Steady-state processes maintain a constant internal energy.
    • Quasistatic processes occur slowly enough that the system reaches equilibrium between infinitesimal disturbances.
    • Spontaneous processes occur without an energy source.
    • Reversible processes are quasistatic and can be reversed.
    • Irreversible processes are not quasistatic or involve frictional or dissipative forces.

    P-V Diagrams

    • Work done in thermal physics can be calculated in two common ways:
      • Expressing pressure as a function of volume and integrating.
      • Finding the area under the curve for a P-V diagram.
    • The area under the curve for a P-V diagram represents work done.
      • Positive area indicates an increase in volume.
      • Negative area indicates a decrease in volume.

    Thermodynamic Processes

    • Isochoric Process:
      • Volume remains constant (∆𝑉 = 0).
      • No work is done (𝑊 = 0).
      • Heat exchange is expressed in terms of specific heat capacity at constant volume.
      • Change in internal energy equals heat exchanged (∆𝑈 = 𝑄).
    • Isobaric Process:
      • Pressure remains constant.
      • Work is calculated using the integral 𝑊 = ∫𝑉=𝑉 𝑃𝑑𝑉 = 𝑃 (𝑉 − 𝑉𝑜 ) = 𝑃∆𝑉.
      • Heat exchange is expressed in terms of specific heat capacity at constant pressure.
      • Internal energy change is ∆𝑈 = 𝑄 − 𝑊.
    • Free Expansion:
      • Occurs under zero pressure.
      • No work is done (𝑊 = 0) because the pressure equals zero.
      • Change in internal energy equals heat exchanged: ∆𝑈 = 𝑄.
    • Isothermal Process:
      • Temperature remains constant.
      • Heat change (𝑄 = 𝑛𝑐𝑉 ∆𝑇) depends on the molar specific heat at constant volume.
      • Internal energy change (∆𝑈 = 𝑄 − 𝑊) can be simplified for different scenarios.
      • For an isochor, ∆𝑈 = 𝑄 = 𝑛𝑐𝑉 ∆𝑇. Internal energy depends only on temperature.
      • For an isobar, 𝑊 = 𝑛𝑅∆𝑇. Heat change depends on the molar specific heat at constant pressure.
      • Internal energy change is ∆𝑈 = 𝑛𝑐𝑃 ∆𝑇 − 𝑛𝑅∆𝑇.
      • For a monatomic ideal gas, 𝑐𝑉 = 𝑅, 𝑐𝑝 = 𝑅, and 𝛾 = 5/3.
    • Adiabatic Process:
      • No heat absorption or release takes place.
      • The relationship between pressure and volume can be expressed as 𝑃𝑜 𝑉𝑜 = 𝑃𝑉𝜸 for an ideal gas.
      • This relationship can be derived by combining the ideal gas law and the first law of thermodynamics.

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