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Questions and Answers
In an isobaric process, which variable remains constant throughout the process?
In which scenario would the isobaric process typically be considered?
What is the work done during an isochoric process?
For an isothermal process involving an ideal gas, what is the change in internal energy?
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What is the relationship between pressure and volume for an isothermal process?
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Which statement about the change in enthalpy (DH) during an isothermal process involving ideal gas is correct?
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What characterizes an ideal gas during isothermal and isobaric processes?
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Why is the work done during an isothermal reversible process greater than that in an adiabatic process?
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What does a negative sign for dV indicate during compression?
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What unit of work corresponds to 1 atm × litre?
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What does the work done (dW) equate to in relation to pressure and volume changes?
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In terms of heat, what does a positive sign represent?
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How does the internal energy of a system change when it gains energy from the surroundings?
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What is the relationship between calories and joules based on the given conversions?
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What happens to the temperature of a system when it acquires energy from a cooler surrounding?
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During expansion, how is work done characterized?
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Which statement about internal energy is true?
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Why can't the absolute value of internal energy be calculated?
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Which of the following describes an extensive property?
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What is the relationship between internal energy and pressure for 1 mole of an ideal gas?
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Which of the following statements regarding thermal equilibrium is correct?
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Which type of thermodynamic property is independent of mass?
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What aspect of a cyclic process prevents a change in internal energy?
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Which of the following types of energy is excluded from the calculation of internal energy?
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What is the system type for a helium-filled balloon?
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Which is an example of an extensive property?
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What type of macroscopic energy changes are complexities not included in internal energy?
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What type of thermodynamic system is represented by a refrigerator cycle?
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Which of the following is an example of an intensive property?
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Which of the following statements about extensive properties is true?
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What characterizes a thermodynamic state function?
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Which of the following is NOT an intensive property?
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What is the work done in cal during the reaction of 260 g Zn with HCl?
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In the equation, W = -2303 nRT log H, what does 'n' represent?
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What is the final temperature after the change of 22 gm CO2 from 500 ml, 300 K to 4L?
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What does the term Dng represent in the context of the reactions?
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What is the work done in cal when 22 gm CO2 changes under reversible and adiabatic conditions?
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In the reaction equation Zn (s) + 2HCl (l) → ZnCl2 (s) + H2 (g), how many moles of Zn are represented by 260 g?
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What is the value of R in the work done equation W = DngRT?
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How is the total work done calculated during gas expansion within a system?
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Study Notes
Internal Energy
- Internal energy (E or U) is the sum of various types of energies associated with a system.
- Internal energy includes potential energy, kinetic energy, thermal energy, and other forms of energy.
- Gravitational potential energy is not considered part of internal energy.
- Calculating the absolute value of internal energy is impossible because it's challenging to determine the exact value of all energy types at a given time.
- Internal energy is an extensive property, meaning it depends on the amount of matter in the system.
- Internal energy is a state function, meaning its value depends solely on the system's current state, not the path it took to reach that state.
Ideal Gas Internal Energy
- For one mole of an ideal gas, internal energy (U) is equal to kinetic energy (KE) and is expressed as 3/2 * RT, where R is the ideal gas constant and T is the temperature.
Thermodynamic Processes
-
Isobaric Process: A process occurring at constant pressure.
- Pressure remains constant (ΔP = 0).
- Work done (W) is calculated as W = PΔV, where P is the constant pressure and ΔV is the change in volume.
-
Isochoric Process: A process occurring at constant volume.
- Volume remains constant (ΔV = 0).
- Work done (W) is zero.
-
Isothermal Process: A process occurring at constant temperature.
- Temperature remains constant (ΔT = 0).
- For ideal gases, the change in internal energy (ΔU) is zero during an isothermal process.
- For ideal gases with constant moles, the change in enthalpy (ΔH) is also zero.
Work Done
- Work done on a system is positive during compression.
- Work done by a system is negative during expansion.
- The unit of work is atmosphere-liter (atm × liter).
- 1 atm × liter = 101.3 J = 24.23 cal.
Heat
- Heat (Q) is the energy transferred between bodies due to a temperature difference.
- Heat absorbed by the system is represented as positive (+).
- Heat evolved by the system is represented as negative (-).
Systems and Surroundings
- An isolated system does not exchange energy or matter with its surroundings.
- An open system exchanges both energy and matter with its surroundings.
- A closed system exchanges energy but not matter with its surroundings.
Thermodynamic Properties
- Intensive properties are independent of the system's mass, remain uniform throughout the system, and are non-additive.
- Extensive properties depend on the system's mass, are additive, and their ratio can form an intensive property.
- State functions are thermodynamic properties that depend only on the system's initial and final states, not the path taken between them.
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Description
Explore the concept of internal energy in thermodynamics, including its components such as potential and kinetic energy. This quiz covers key principles related to the internal energy of ideal gases and various thermodynamic processes. Test your understanding of how internal energy functions as a state property and its implications in different scenarios.