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To help derive the relationships shown in the various gas laws, you will be using an interactive research- based simulation produced by the PhET project at the University of Colorado.

To help derive the relationships shown in the various gas laws, you will be using an interactive research- based simulation produced by the PhET project at the University of Colorado.

General Chemistry - Standalone book (MindTap Course List)
General Chemistry - Standalone book (MindTap Course List)
11th Edition
ISBN:9781305580343
Author:Steven D. Gammon, Ebbing, Darrell Ebbing, Steven D., Darrell; Gammon, Darrell Ebbing; Steven D. Gammon, Darrell D.; Gammon, Ebbing; Steven D. Gammon; Darrell
Publisher:Steven D. Gammon, Ebbing, Darrell Ebbing, Steven D., Darrell; Gammon, Darrell Ebbing; Steven D. Gammon, Darrell D.; Gammon, Ebbing; Steven D. Gammon; Darrell
Chapter5: The Gaseous State
Section: Chapter Questions
Problem 5.17QP
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Concept overview According to the kinetic molecular theory, gasses are in constant and random motion with enough kinetic energy such that they rarely interact with one another. When gas particles collide with the walls of a container, they rebound with no apparent loss of energy. These characteristics describe an "Ideal Gas". Experimental evidence suggests that many common gasses making up air behave in this manner when studied at temperatures well above their boiling points. We are constantly being exposed to the behavior of gasses. Each time we pump up a tire, blow up a balloon, use a spray can, or experience the cooling of gasses as they escape from a gas storage container, we are reminded of how gasses behave with changes in temperature (T), volume (V), pressure (P), or number of particles (n). The behavior of gasses has been scientifically investigated starting with Robert Boyle's work in 1662, followed by Jacques Charles' (1787) and Joseph Gay-Lussac's work (1802). Together these studies led to the so-called "Gas Laws" which relate volume (V), pressure (P), temperature (T) and numbers of particles of gas (n). In a scientific manner, one can derive the mathematical relationships that exist between these variables by holding two of the variable's constant, changing one, and monitoring the effect on the fourth variable. When dealing with mixtures of gasses, John Dalton postulated the Law of Partial Pressures, which indicates that at constant temperature, the pressure of a mixture of gasses is the sum of the pressures of the gasses, measured separately, in the same container. This indicates that when working with a mixture of gasses, it is easy to discount one from another when using the other gas laws. To help derive the relationships shown in the various gas laws, you will be using an interactive research- based simulation produced by the PhET project at the University of Colorado.
Transcribed Image Text:Concept overview According to the kinetic molecular theory, gasses are in constant and random motion with enough kinetic energy such that they rarely interact with one another. When gas particles collide with the walls of a container, they rebound with no apparent loss of energy. These characteristics describe an "Ideal Gas". Experimental evidence suggests that many common gasses making up air behave in this manner when studied at temperatures well above their boiling points. We are constantly being exposed to the behavior of gasses. Each time we pump up a tire, blow up a balloon, use a spray can, or experience the cooling of gasses as they escape from a gas storage container, we are reminded of how gasses behave with changes in temperature (T), volume (V), pressure (P), or number of particles (n). The behavior of gasses has been scientifically investigated starting with Robert Boyle's work in 1662, followed by Jacques Charles' (1787) and Joseph Gay-Lussac's work (1802). Together these studies led to the so-called "Gas Laws" which relate volume (V), pressure (P), temperature (T) and numbers of particles of gas (n). In a scientific manner, one can derive the mathematical relationships that exist between these variables by holding two of the variable's constant, changing one, and monitoring the effect on the fourth variable. When dealing with mixtures of gasses, John Dalton postulated the Law of Partial Pressures, which indicates that at constant temperature, the pressure of a mixture of gasses is the sum of the pressures of the gasses, measured separately, in the same container. This indicates that when working with a mixture of gasses, it is easy to discount one from another when using the other gas laws. To help derive the relationships shown in the various gas laws, you will be using an interactive research- based simulation produced by the PhET project at the University of Colorado.
1. In a mixture of three gasses (A, B, and C), explain how are the partial pressures of the gasses related to the total pressure of the mixture? 2. Equal molar quantities of two gasses of molecular weight 4 and 40 are mixed. The pressure of the mixture is 1.2 atm. What is the partial pressure of the lighter gas in this mixture? Explain. 3. When gasses are collected by water displacement, there is always water vapor (gaseous water) present. The amount of water vapor present depends on the temperature. The greater the temperature, the more water vapor present (this quantity is called the vapor pressure). A 1.00 L volume of nitrogen gas measured at 290 K and 0.978 atm was collected at 290 K by water displacement. Use Dalton's Law and the Ideal Gas Law to determine the number of moles of nitrogen gas that were collected. At 290 K, the vapor pressure of water is 14.59 Torr.
Transcribed Image Text:1. In a mixture of three gasses (A, B, and C), explain how are the partial pressures of the gasses related to the total pressure of the mixture? 2. Equal molar quantities of two gasses of molecular weight 4 and 40 are mixed. The pressure of the mixture is 1.2 atm. What is the partial pressure of the lighter gas in this mixture? Explain. 3. When gasses are collected by water displacement, there is always water vapor (gaseous water) present. The amount of water vapor present depends on the temperature. The greater the temperature, the more water vapor present (this quantity is called the vapor pressure). A 1.00 L volume of nitrogen gas measured at 290 K and 0.978 atm was collected at 290 K by water displacement. Use Dalton's Law and the Ideal Gas Law to determine the number of moles of nitrogen gas that were collected. At 290 K, the vapor pressure of water is 14.59 Torr.
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