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CHM 112 > Chpt 2 Kinetic Molecular Theory > Flashcards

Chpt 2 Kinetic Molecular Theory Flashcards

1
Q

QUESTION

A

OPTION 1

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2
Q
  1. (What does the kinetic-molecular theory postulate about heat? A. Heat only depends on rotational motion B. Heat is unrelated to molecular motion C. Heat is a manifestation of molecular motion D. Heat is independent of temperature)
A

Answer: C. Heat is a manifestation of molecular motion

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3
Q
  1. (Which of the following is NOT a basic assumption of the kinetic-molecular theory? A. Gas molecules are far apart in empty space B. Molecules are perfectly inelastic C. Molecules are in rapid, random motion D. Gas pressure arises from molecular collisions)
A

Answer: B. Molecules are perfectly inelastic

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4
Q
  1. (What does the average kinetic energy of gas molecules depend on? A. Absolute temperature B. Type of gas C. Volume of the gas D. Size of the container)
A

Answer: A. Absolute temperature

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5
Q
  1. (Why are gases highly compressible according to the kinetic theory? A. Molecules form dense clusters B. Gas molecules are incompressible C. Most of the gas volume is empty space D. Molecules resist pressure)
A

Answer: C. Most of the gas volume is empty space

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6
Q
  1. (Which equation represents the ideal gas law? A. B. C. D.)
A

Answer: (No options provided)

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7
Q
  1. (How does molecular impact contribute to gas pressure? A. By compressing molecules closer together B. Through cumulative collisions with container walls C. By transferring heat to the container D. By causing elastic deformation of molecules)
A

Answer: B. Through cumulative collisions with container walls

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8
Q
  1. (What is the relationship between pressure (P), volume (V), and temperature (T) in an ideal gas? A. B. C. D.)
A

Answer: (No options provided)

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9
Q
  1. (In the ideal gas law, represents which of the following? A. Universal gas constant B. Boltzmann constant C. Mole ratio constant D. Diffusion constant)
A

Answer: A. Universal gas constant

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10
Q
  1. (What does Dalton’s law of partial pressures state? A. Total pressure equals the sum of individual gas pressures B. Total pressure equals the average molecular velocity C. Total pressure is inversely proportional to volume D. Total pressure depends only on the heaviest gas)
A

Answer: A. Total pressure equals the sum of individual gas pressures

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11
Q
  1. (What assumption is unique to the ideal gas model? A. Molecules exert no attraction on each other B. Molecular volume is significant C. Kinetic energy is rotational D. Molecules move in preferred directions)
A

Answer: A. Molecules exert no attraction on each other

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12
Q
  1. (What is the average kinetic energy of one mole of gas proportional to? A. B. C. D.)
A

Answer: (No options provided)

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13
Q
  1. (Which gas law relates pressure and volume at constant temperature? A. Boyle’s law B. Charles’s law C. Avogadro’s law D. Dalton’s law)
A

Answer: A. Boyle’s law

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14
Q
  1. (How is the mean square velocity of a gas molecule represented? A. B. C. D.)
A

Answer: (No options provided)

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15
Q
  1. (According to Graham’s law of diffusion, the rate of diffusion is inversely proportional to: A. Square root of molar mass B. Temperature C. Molecular collision number D. Gas pressure)
A

Answer: A. Square root of molar mass

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16
Q
  1. (What does Avogadro’s principle state about equal volumes of gases? A. They contain equal numbers of molecules at the same temperature and pressure B. They have identical masses C. They have identical densities D. They have equal kinetic energies)
A

Answer: A. They contain equal numbers of molecules at the same temperature and pressure

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17
Q
  1. (What is the distribution of molecular speeds in a gas represented by? A. A Gaussian distribution B. The Maxwell-Boltzmann distribution C. A probability density function D. A uniform distribution)
A

Answer: C. A probability density function

18
Q
  1. (Which of the following represents the most probable speed of molecules in a gas? A. The mean speed of all molecules B. The speed corresponding to the maximum of the speed distribution curve C. The average velocity of molecules D. The speed at which half of the molecules move faster)
A

Answer: B. The speed corresponding to the maximum of the speed distribution curve

19
Q
  1. (What happens to the most probable speed as temperature increases? A. It stays constant B. It decreases C. It increases D. It becomes zero)
A

Answer: C. It increases

20
Q
  1. (In the kinetic theory of gases, the probability of a molecule having a speed between c and e + de is given by which equation? A. Equation 2.21 B. Equation 2.28 C. Equation 2.16 D. Equation 2.24)
A

Answer: B. Equation 2.28

21
Q
  1. (Which of the following factors affects the speed distribution of gas molecules? A. Temperature B. Molecular mass C. Pressure D. Volume)
A

Answer: A. Temperature

22
Q
  1. (The velocity distribution of molecules in the X, Y, and Z directions is: A. Dependent on the gas type B. Identical C. Different in each direction D. Not defined)
A

Answer: B. Identical

23
Q
  1. (What is the root-mean-square speed of molecules defined as? A. The arithmetic mean of the speeds B. The most probable speed C. The square root of the average of the squares of molecular speeds D. The average velocity of all molecules)
A

Answer: C. The square root of the average of the squares of molecular speeds

24
Q
  1. (The arithmetic mean speed is obtained by: A. Averaging the speeds of molecules at different temperatures B. Taking the maximum of the speed distribution curve C. Summing all the speeds and dividing by the total number of molecules D. Taking the square root of the average squared speed)
A

Answer: C. Summing all the speeds and dividing by the total number of molecules

25
Q
  1. (The root-mean-square speed for hydrogen molecules at 0°C is approximately: A. 1694 m/s B. 1250 m/s C. 1838 m/s D. 1500 m/s)
A

Answer: A. 1838 m/s

26
Q
  1. (What does the equation represent in the context of the kinetic theory of gases? A. The kinetic energy of a molecule B. The root-mean-square speed C. The most probable speed D. The arithmetic mean speed)
A

Answer: A. The kinetic energy of a molecule

27
Q
  1. (What is the average kinetic energy of one molecule in an ideal gas? A. B. C. D.)
A

Answer: (No options provided)

28
Q
  1. (For a given temperature, which molecules will have the highest speeds? A. Lighter molecules B. Heavier molecules C. Molecules with higher densities D. Molecules with higher volumes)
A

Answer: A. Lighter molecules

29
Q
  1. (The kinetic energy of a gas molecule depends primarily on: A. Temperature B. Molecular weight C. Pressure D. Volume)
A

Answer: A. Temperature

30
Q
  1. (The relationship between temperature and the root-mean-square speed of a gas molecule is: A. Unrelated B. Inversely proportional C. Exponentially related D. Directly proportional)
A

Answer: D. Directly proportional

31
Q
  1. (At higher temperatures, the distribution of speeds of gas molecules: A. Becomes narrower B. Becomes broader C. Remains the same D. Shifts to lower speeds)
A

Answer: B. Becomes broader

32
Q
  1. (The probability that a molecule has a speed between two values is given by: A. The area under the speed distribution curve B. The maximum of the speed distribution C. The arithmetic mean of speeds D. The velocity distribution in the X direction)
A

Answer: A. The area under the speed distribution curve

33
Q
  1. (The velocity probability distribution curve for molecules in the X-direction shows: A. Zero most probable velocity B. An exponential decay with increasing speed C. A single peak at high speeds D. Equal probabilities for positive and negative velocities)
A

Answer: D. Equal probabilities for positive and negative velocities

34
Q
  1. (Which of the following molecular speeds is most likely to be found in a gas? A. Most probable speed B. Root-mean-square speed C. Arithmetic mean speed D. Average velocity)
A

Answer: A. Most probable speed

35
Q
  1. (What type of gas molecules would have lower average speeds at a given temperature? A. Heavier molecules B. Lighter molecules C. More energetic molecules D. Molecules with higher kinetic energy)
A

Answer: A. Heavier molecules

36
Q
  1. (The average kinetic energy of gas molecules in an ideal gas is: A. Independent of volume and pressure B. Dependent on molecular mass C. Proportional to the pressure of the gas D. Proportional to the volume of the container)
A

Answer: A. Independent of volume and pressure

37
Q
  1. (The most probable speed for oxygen molecules at 0°C is: A. Higher than that of hydrogen molecules at 0°C B. Lower than that of hydrogen molecules at 0°C C. The same as that of hydrogen molecules at 0°C D. Independent of the temperature)
A

Answer: A. Higher than that of hydrogen molecules at 0°C

38
Q
  1. (At a given temperature, which type of gas will have the greatest average speed? A. A light gas like hydrogen B. A monoatomic gas C. A diatomic gas like nitrogen D. A heavy gas like xenon)
A

Answer: A. A light gas like hydrogen

39
Q
  1. (Which of the following expressions relates to the root-mean-square speed of gas molecules? A. B. C. D.)
A

Answer: (No options provided)

40
Q
  1. (The most probable velocity of a gas molecule is: A. The peak of the velocity distribution B. The square root of the mean square speed C. The average speed of all molecules D. Always zero for ideal gases)
A

Answer: A. The peak of the velocity distribution

41
Q
  1. (The speed distribution of gas molecules at a given temperature is: A. A function of temperature and molecular mass B. Only influenced by the molecular weight C. Only influenced by the volume of the container D. Independent of temperature)
A

Answer: A. A function of temperature and molecular mass

CHM 112 (7 decks)

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