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IMU CET Gases — practice questions — page 4

Explore 97 free Gases questions in IMU CET Chemistry. Open each question or exercise to read its content, reference answers and available explanation.

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Gases questions and exercises with answers

Showing questions 91–97 of 97.

Kinetic molecular theory explains Boyle's law by which change when the volume of a gas decreases?Read the answer and worked solution →For a gas showing perfectly ideal behaviour, the compressibility factor Z takes which value?Read the answer and worked solution →Under which conditions does a real gas behave most nearly like an ideal gas?Read the answer and worked solution →Who developed the first and simplest equation that improves on the ideal gas law?Read the answer and worked solution →In the van der Waals equation, what does the constant b account for?Read the answer and worked solution →A 4.25 L flask holds 3.46 mol of carbon dioxide at 229 degrees C. What pressure does the ideal gas law predict?Read the answer and worked solution →The van der Waals equation reduces to PV = nRT under which condition?Read the answer and worked solution →

Worked practice questions

Kinetic molecular theory explains Boyle's law by which change when the volume of a gas decreases?

  1. Molecules lose kinetic energy quickly
  2. Wall collisions become more frequent
  3. Molecules begin to attract each other
  4. The average molecular speed increases
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Correct answer: B. Wall collisions become more frequent

1. Squeezing a gas into a smaller space shortens the distance a molecule travels before it meets a wall. 2. Collisions with the walls therefore happen more often, and the wall area they are spread over has also shrunk. 3. Both effects push the pressure up, which is exactly what Boyle's law records. 4. The temperature has not changed, so the average speed and kinetic energy of the molecules stay the same throughout. _Source: OpenStax Chemistry (CC BY 4.0), Ch 9 "Gases", section 9.5 The Kinetic-Molecular Theory_

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For a gas showing perfectly ideal behaviour, the compressibility factor Z takes which value?

  1. Zero exactly
  2. Always above 1
  3. One exactly
  4. Always below 1
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Correct answer: C. One exactly

1. The compressibility factor compares the real molar volume of a gas with the molar volume an ideal gas would have at the same temperature and pressure. 2. If the gas behaves ideally the two volumes match and the ratio is exactly 1. 3. Any departure from 1, in either direction, signals non-ideal behaviour. 4. Real gases dip below 1 at moderate pressures because of attractions, then climb above 1 at very high pressures because of molecular volume. _Source: OpenStax Chemistry (CC BY 4.0), Ch 9 "Gases", section 9.6 Non-Ideal Gas Behavior_

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Under which conditions does a real gas behave most nearly like an ideal gas?

  1. High pressure and low temperature
  2. High pressure and high temperature
  3. Low pressure and low temperature
  4. Low pressure and high temperature
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Correct answer: D. Low pressure and high temperature

1. The ideal gas equation works when molecular attractions can be ignored and the molecules take up no appreciable share of the volume. 2. Low pressure spreads the molecules far apart, so their own volume is a tiny fraction of the total and attractions barely act. 3. High temperature gives them enough kinetic energy to shrug off whatever attractions remain. 4. Low temperature and high pressure together are the worst case, since crowded slow molecules both attract and take up room. _Source: OpenStax Chemistry (CC BY 4.0), Ch 9 "Gases", section 9.6 Non-Ideal Gas Behavior_

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