F10HW7-CH5 - HOMEWORK WEEK 7 CHAPTER 5 5.15 This question...

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HOMEWORK WEEK 7 CHAPTER 5 5.15 This question applies to ideal gases. The postulates and supporting evidence are the following: (1) Gases are composed of molecules whose sizes are negligible compared with the distance between them. (2) Molecules move randomly in straight lines in all directions and at various speeds. (3) The forces of attraction or repulsion between two molecules (intermolecular forces) in a gas are very weak or negligible, except when they collide. (4) When molecules collide with one another, the collisions are elastic. (5) The average kinetic energy of a molecule is proportional to the absolute temperature. One example of evidence that supports the kinetic theory of gases is Boyle’s law. Constant temperature means the average molecular force from collision remains constant. If you increase the volume, you decrease the number of collisions per unit wall area, thus lowering the pressure in accordance with Boyle’s law. Another example is Charles’s law. If you raise the temperature, you increase the average molecular force from a collision with the wall, thus increasing the pressure. For the pressure to remain constant, it is necessary for the volume to increase so the frequency of collisions with the wall decreases. Thus, when you raise the temperature of a gas while keeping the pressure constant, the volume increases in accordance with Charles’s law. 5.17 According to kinetic theory, the pressure of a gas results from the forces arising from the bombardment of container walls by molecules. 5.20 Effusion is the process in which a gas flows through a small hole in a container. It results from the gas molecules encountering the hole by chance, rather than by colliding with another part of the walls of the container. The faster the molecules move, the greater the frequency of collisions with the wall and thus also with the hole. Thus, the rate of effusion depends on the average molecular speed, which depends inversely on molecular mass. 010. The answer is a; “the greater the volume occupied by a given amount of gas, the higher the intermolecular force” is incorrect. The magnitude of the force is independent of volume and the effect of the force diminishes as volume increases. 5.29 a. The volume of the tire and the amount of air in the tire remain constant. From the ideal
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This note was uploaded on 02/20/2011 for the course CHEM 110 taught by Professor Dr.huston during the Spring '06 term at Pittsburgh.

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F10HW7-CH5 - HOMEWORK WEEK 7 CHAPTER 5 5.15 This question...

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