Chemistry Exam > Chemistry Questions > Consider the following statements:(I) The wor...
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Consider the following statements:
(I) The work done in the reversible isothermal expansion of an ideal gas is greater than that for Vander Waals Gas
(II) When an ideal gas undergoes adiabatic expansion, internal energy increases Which of the statement is true?
(II) When an ideal gas undergoes adiabatic expansion, internal energy increases Which of the statement is true?
- a)I only
- b)II only
- c)Both I and II
- d)Neither I and II
Correct answer is option 'A'. Can you explain this answer?
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Most Upvoted Answer
Consider the following statements:(I) The work done in the reversible ...
Reversible Isothermal Expansion of Ideal Gas vs Vander Waals Gas
- In the reversible isothermal expansion, the temperature is kept constant, and the gas expands or contracts slowly and reversibly. The work done during this process can be calculated using the formula W = -nRTln(V2/V1) where n is the number of moles of gas, R is the gas constant, T is the temperature, and V1 and V2 are the initial and final volumes of the gas.
- The work done in the reversible isothermal expansion of an ideal gas is greater than that for Vander Waals Gas because the Vander Waals gas has intermolecular forces that cause it to deviate from the ideal gas law. These forces create an additional energy barrier that must be overcome during the expansion, leading to less work being done.
- Therefore, statement (I) is true.
Adiabatic Expansion of Ideal Gas
- In an adiabatic expansion, no heat is exchanged between the gas and its surroundings. The internal energy of the gas changes due to the work done during the expansion, but the temperature of the gas may change as well.
- For an ideal gas, the internal energy depends only on the temperature, so if the temperature remains constant, the internal energy will not change. Therefore, statement (II) is false.
- However, for a real gas, the internal energy may change even if the temperature remains constant due to intermolecular forces. This is known as the Joule-Thomson effect.
Overall, the correct answer is (A) I only.
- In the reversible isothermal expansion, the temperature is kept constant, and the gas expands or contracts slowly and reversibly. The work done during this process can be calculated using the formula W = -nRTln(V2/V1) where n is the number of moles of gas, R is the gas constant, T is the temperature, and V1 and V2 are the initial and final volumes of the gas.
- The work done in the reversible isothermal expansion of an ideal gas is greater than that for Vander Waals Gas because the Vander Waals gas has intermolecular forces that cause it to deviate from the ideal gas law. These forces create an additional energy barrier that must be overcome during the expansion, leading to less work being done.
- Therefore, statement (I) is true.
Adiabatic Expansion of Ideal Gas
- In an adiabatic expansion, no heat is exchanged between the gas and its surroundings. The internal energy of the gas changes due to the work done during the expansion, but the temperature of the gas may change as well.
- For an ideal gas, the internal energy depends only on the temperature, so if the temperature remains constant, the internal energy will not change. Therefore, statement (II) is false.
- However, for a real gas, the internal energy may change even if the temperature remains constant due to intermolecular forces. This is known as the Joule-Thomson effect.
Overall, the correct answer is (A) I only.
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Consider the following statements:(I) The work done in the reversible isothermal expansion of an ideal gas is greater than that for Vander Waals Gas(II) When an ideal gas undergoes adiabatic expansion, internal energy increases Which of the statement is true?a)I onlyb)II onlyc)Both I and IId)Neither I and IICorrect answer is option 'A'. Can you explain this answer?
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