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7. Gases

Kinetic Molecular Theory

7. Gases

Kinetic Molecular Theory

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Kinetic Molecular Theory

Kinetic Molecular Theory

Kinetic Molecular Theory Example 1

Kinetic Molecular Theory Example 1

Kinetic Molecular Theory

Kinetic Molecular Theory

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Multiple Choice

Which of the following statements would correctly explain the non-ideal behavior of a gas based on the Kinetic Molecular Theory (KMT)?

a) At high temperatures the attractive forces between molecules becomes negligible.
b) At high pressure the volume of gas molecules become significant.
c) An increase or decrease in the moles of gas causes the gas constant value to change.

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Multiple Choice

Which of the following statements is/are true for gas molecules according to the Kinetic Molecular Theory?

I.Increasing the amount of gas molecules increases the pressure by increasing the force of the collisions.
II.Decreasing the temperature of a gas decreases the pressure by increasing the force of the collisions.
III.Decreasing the volume of a gas increases pressure by increasing the frequency of the collisions.

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Multiple Choice

Based on the kinetic-molecular theory, which of the following is/are true?
I.At a given temperature, all gases have the same average kinetic energy.
II.At a given temperature, different gases have the same average velocities.
III.The average kinetic energy is proportional to the absolute temperature.

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Multiple Choice

Which statement is TRUE about kinetic molecular theory?

a) A single particle does not move in a straight line.
b) The size of the particle is large compared to the volume.
c) The collisions of particles with one another is completely elastic.
d) The average kinetic energy of a particle is not proportional to the temperature.

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Textbook Question

At 273 K and 1 atm pressure, 1 mol of an ideal gas occupies 22.4 L. (Section 10.4) (c) In which parts of the atmosphere would you expect gases to behave most ideally (ignoring any photochemical reactions)? [Section 18.1]

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Textbook Question

(c) What happens to a gas if you put it under extremely high pressure?

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Textbook Question

Identify the true statement about deviations from ideal gas behavior. (LO 10.12) (a) The attractive forces between gas particles cause the true volume of the sample to be larger than predicted by the ideal gas law. (b) The attractive forces between gas particles most influence the volume of a sample at low pressure. (c) The volume of the gas particles themselves most influences the volume of the sample at low pressure. (d) The volume of the gas particles themselves causes the true volume of the sample to be larger than predicted by the ideal gas law.

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Textbook Question

Which of the following statements is false? (a) Gases are far less dense than liquids. (b) Gases are far more compressible than liquids. (c) Because liquid water and liquid carbon tetrachloride do not mix, neither do their vapors. (d) The volume occupied by a gas is determined by the volume of its container.

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Textbook Question

Which of the following statements best explains why a closed balloon filled with helium gas rises in air? (a) Helium is a monatomic gas, whereas nearly all the molecules that make up air, such as nitrogen and oxygen, are diatomic. (b) The average speed of helium atoms is greater than the average speed of air molecules, and the greater speed of collisions with the balloon walls propels the balloon upward. (c) Because the helium atoms are of lower mass than the average air molecule, the helium gas is less dense than air. The mass of the balloon is thus less than the mass of the air displaced by its volume. (d) Because helium has a lower molar mass than the average air molecule, the helium atoms are in faster motion. This means that the temperature of the helium is greater than the air temperature. Hot gases tend to rise.

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Textbook Question

Determine whether each of the following changes will increase, decrease, or not affect the rate with which gas molecules collide with the walls of their container: (a) increasing the volume of the container (b) increasing the temperature (c) increasing the molar mass of the gas

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Textbook Question

Indicate which of the following statements regarding the kinetic-molecular theory of gases are correct. (a) The average kinetic energy of a collection of gas molecules at a given temperature is proportional to m1>2.

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Textbook Question

The temperature of a 5.00-L container of N2 gas is increased from 20 °C to 250 °C. If the volume is held constant, predict qualitatively how this change affects the following: (a) the average kinetic energy of the molecules.

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Textbook Question

At constant pressure, the mean free path 1l2 of a gas molecule is directly proportional to temperature. At constant temperature, l is inversely proportional to pressure. If you compare two different gas molecules at the same temperature and pressure, l is inversely proportional to the square of the diameter of the gas molecules. Put these facts together to create a formula for the mean free path of a gas molecule with a proportionality constant (call it Rmfp, like the ideal-gas constant) and define units for Rmfp.

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Textbook Question

(b) List two reasons why the gases deviate from ideal behavior.

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Textbook Question

The planet Jupiter has a surface temperature of 140 K and a mass 318 times that of Earth. Mercury (the planet) has a surface temperature between 600 K and 700 K and a mass 0.05 times that of Earth. On which planet is the atmosphere more likely to obey the ideal-gas law? Explain.

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Textbook Question

Which postulate of the kinetic molecular theory breaks down under conditions of high pressure? Explain.

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Textbook Question

What are the basic assumptions of the kinetic–molecular theory?

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Textbook Question

The phase diagram for SO2 is shown here. (e) At which of the three red points does SO21g2 behave least ideally?

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Textbook Question

The phase diagram for SO2 is shown here. (d) At which of the three points marked in red does SO21g2 most closely approach ideal-gas behavior?

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Textbook Question

Two 112-L tanks are filled with gas at 330 K. One contains 5.00 mol of Kr, and the other contains 5.00 mol of O2. Considering the assumptions of kinetic–molecular theory, rank the gases from low to high for each of the following properties. (d) Pressure

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Textbook Question

Two 112-L tanks are filled with gas at 330 K. One contains 5.00 mol of Kr, and the other contains 5.00 mol of O2. Considering the assumptions of kinetic–molecular theory, rank the gases from low to high for each of the following properties. (a) Collision frequency

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Textbook Question

Consider the following gases, all at STP: Ne, SF6, N2, CH4. (a) Which gas is most likely to depart from the assumption of the kinetic-molecular theory that says there are no attractive or repulsive forces between molecules?

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Which temperature represents the highest average kinetic energy?

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Which of the gases has the fastest‑moving molecules, on average, at a given temperature?

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