Chemistry Exam > Chemistry Questions > Select the correct statement(s):a)At Boyles t...
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Select the correct statement(s):
- a)At Boyle’s temperature a real gas behaves like an ideal gas at low pressure
- b)Above critical conditions, a real gas behave like an ideal gas
- c)For hydrogen gas ‘b’ dominates over ‘a’ at all temperature
- d)At high pressure van der Waal’s constant ‘b’ dominates over ‘a’
Correct answer is option 'D'. Can you explain this answer?
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Most Upvoted Answer
Select the correct statement(s):a)At Boyles temperature a real gas beh...
At Boyle's temperature, a real gas behaves like an ideal gas at low pressure.
Above critical conditions, a real gas behaves like an ideal gas.
For hydrogen gas, 'b' dominates over 'a' at only room temperature and pressure.
At high-pressure van der Waals's constant 'b' dominates over 'a'.
Hence, Options "A", "B" & "D" are correct answers.
Above critical conditions, a real gas behaves like an ideal gas.
For hydrogen gas, 'b' dominates over 'a' at only room temperature and pressure.
At high-pressure van der Waals's constant 'b' dominates over 'a'.
Hence, Options "A", "B" & "D" are correct answers.
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Select the correct statement(s):a)At Boyles temperature a real gas beh...
Understanding Real Gases and Ideal Gas Behavior
Real gases deviate from ideal behavior under certain conditions. The van der Waals equation accounts for these deviations by introducing two constants, 'a' and 'b', which represent molecular interactions and volume occupied by gas molecules, respectively.
Explanation of Option D
- At high pressures, gas molecules are forced closer together, leading to significant intermolecular interactions.
- In this scenario, the volume occupied by the gas molecules (represented by 'b') becomes increasingly important and cannot be neglected.
- The term 'b' dominates over 'a' because the volume exclusion effect becomes more pronounced as the pressure increases.
- Conversely, the attractive forces represented by 'a' become less significant compared to the volume exclusions caused by the finite size of the gas molecules.
Clarification of Other Options
- Option A: Boyle's Temperature
- At Boyle's temperature, a real gas behaves more like an ideal gas, but only at low pressures. This statement is partially true but does not encompass the whole behavior of real gases.
- Option B: Above Critical Conditions
- Above the critical point, gases do not behave ideally. They show liquid-like properties and significant deviations from ideal behavior.
- Option C: For Hydrogen Gas
- Hydrogen gas does not consistently show 'b' dominating over 'a' at all temperatures. This depends on the conditions and temperature ranges.
Conclusion
In summary, the correct choice is option 'D' due to the dominant effect of the volume occupied by gas molecules at high pressures, which is critical in understanding real gas behavior.
Real gases deviate from ideal behavior under certain conditions. The van der Waals equation accounts for these deviations by introducing two constants, 'a' and 'b', which represent molecular interactions and volume occupied by gas molecules, respectively.
Explanation of Option D
- At high pressures, gas molecules are forced closer together, leading to significant intermolecular interactions.
- In this scenario, the volume occupied by the gas molecules (represented by 'b') becomes increasingly important and cannot be neglected.
- The term 'b' dominates over 'a' because the volume exclusion effect becomes more pronounced as the pressure increases.
- Conversely, the attractive forces represented by 'a' become less significant compared to the volume exclusions caused by the finite size of the gas molecules.
Clarification of Other Options
- Option A: Boyle's Temperature
- At Boyle's temperature, a real gas behaves more like an ideal gas, but only at low pressures. This statement is partially true but does not encompass the whole behavior of real gases.
- Option B: Above Critical Conditions
- Above the critical point, gases do not behave ideally. They show liquid-like properties and significant deviations from ideal behavior.
- Option C: For Hydrogen Gas
- Hydrogen gas does not consistently show 'b' dominating over 'a' at all temperatures. This depends on the conditions and temperature ranges.
Conclusion
In summary, the correct choice is option 'D' due to the dominant effect of the volume occupied by gas molecules at high pressures, which is critical in understanding real gas behavior.
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Select the correct statement(s):a)At Boyles temperature a real gas behaves like an ideal gas at low pressureb)Above critical conditions, a real gas behave like an ideal gasc)For hydrogen gas b dominates over a at all temperatured)At high pressure van der Waals constant b dominates over aCorrect answer is option 'D'. Can you explain this answer?
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