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Learning Goal: To understand the ideal gas law and be able to apply it to a wide variety of situations. The absolute temperature T, volume V, and pressure P of a gas sample are related by the ideal gas law, which states that PV = nRT. Here is the number of moles in the gas sample and R is a gas constant that applies to all gases. This empirical law describes gases well only if they are sufficiently dilute and at a sufficiently high temperature that they are not on the verge of condensing. In applying the ideal gas law, p must be the absolute pressure, measured with respect to vacuum and not with respect to atmospheric pressure, and T must be the absolute temperature. measured in kelvins (that is, with respect to absolute zero, defined throughout this tutorial as -273°C). If p is in pascals and V is in cubic meters, use R 8.3145 J/(mol-K). If p is in atmospheres and V is in liters, use R 0.08206 L atm/(mol- K) instead. Y A gas sample enclosed in a rigid metal container at room temperature (20.0°C) has an absolute pressure pi. The container is immersed in hot water until it warms to 40.0°C. What is the new absolute pressure pa? Express your answer in terms of pi ▸ View Available Hint(s) P2 = 1.07p1 Submit Previous Answers ✓ Correct This modest temperature increase (in absolute terms) leads to a pressure increase of just a few percent. Note that it is critical for the temperatures to be converted to absolute units. If you had used Celsius temperatures. you would have predicted that the pressure should double, which is far greater than the actual increase. Part B Nitrogen gas is introduced into a large deflated plastic bag. No gas is allowed to escape, but as more and more nitrogen is added, the bag inflates to accommodate it. The pressure of the gas within the bag remains at 1.00 atm and its temperature remains at room temperature (20.0°C). How many moles 12 have been introduced into the bag by the time its volume reaches 22.4 L? Express your answer in moles. ▸ View Available Hint(s) 1 Templates Symbols undo regio Reset keyboard shortcuts help W 3.

Learning Goal: To understand the ideal gas law and be able to apply it to a wide variety of situations. The absolute temperature T, volume V, and pressure P of a gas sample are related by the ideal gas law, which states that PV = nRT. Here is the number of moles in the gas sample and R is a gas constant that applies to all gases. This empirical law describes gases well only if they are sufficiently dilute and at a sufficiently high temperature that they are not on the verge of condensing. In applying the ideal gas law, p must be the absolute pressure, measured with respect to vacuum and not with respect to atmospheric pressure, and T must be the absolute temperature. measured in kelvins (that is, with respect to absolute zero, defined throughout this tutorial as -273°C). If p is in pascals and V is in cubic meters, use R 8.3145 J/(mol-K). If p is in atmospheres and V is in liters, use R 0.08206 L atm/(mol- K) instead. Y A gas sample enclosed in a rigid metal container at room temperature (20.0°C) has an absolute pressure pi. The container is immersed in hot water until it warms to 40.0°C. What is the new absolute pressure pa? Express your answer in terms of pi ▸ View Available Hint(s) P2 = 1.07p1 Submit Previous Answers ✓ Correct This modest temperature increase (in absolute terms) leads to a pressure increase of just a few percent. Note that it is critical for the temperatures to be converted to absolute units. If you had used Celsius temperatures. you would have predicted that the pressure should double, which is far greater than the actual increase. Part B Nitrogen gas is introduced into a large deflated plastic bag. No gas is allowed to escape, but as more and more nitrogen is added, the bag inflates to accommodate it. The pressure of the gas within the bag remains at 1.00 atm and its temperature remains at room temperature (20.0°C). How many moles 12 have been introduced into the bag by the time its volume reaches 22.4 L? Express your answer in moles. ▸ View Available Hint(s) 1 Templates Symbols undo regio Reset keyboard shortcuts help W 3.

College Physics
College Physics
11th Edition
ISBN:9781305952300
Author:Raymond A. Serway, Chris Vuille
Publisher:Raymond A. Serway, Chris Vuille
Chapter1: Units, Trigonometry. And Vectors
Section: Chapter Questions
Problem 1CQ: Estimate the order of magnitude of the length, in meters, of each of the following; (a) a mouse, (b)...
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Learning Goal: To understand the ideal gas law and be able to apply it to a wide variety of situations. The absolute temperature T, volume V, and pressure P of a gas sample are related by the ideal gas law, which states that pV=nRT. Here is the number of moles in the gas sample and R is a gas constant that applies to all gases. This empirical law describes gases well only if they are sufficiently dilute and at a sufficiently high temperature that they are not on the verge of condensing. In applying the ideal gas law, p must be the absolute pressure, measured with respect to vacuum and not with respect to atmospheric pressure, and T must be the absolute temperature, measured in kelvins (that is, with respect to absolute zero, defined throughout this tutorial as -273°C). If p is in pascals and V is in cubic meters, use R = 8.3145 J/(mol-K). If p is in atmospheres and V is in liters, use R 0.08206 L atm/(mol-K) instead. A gas sample enclosed in a rigid metal container at room temperature (20.0°C) has an absolute pressure pi. The container is immersed in hot water until it warms to 40.0°C. What is the new absolute pressure p2? Express your answer in terms of p₁. ▸ View Available Hint(s) P2 = 1.07p1 Submit ✓ Correct This modest temperature increase (in absolute terms) leads to a pressure increase of just a few percent. Note that it is critical for the temperatures to be converted to absolute units. If you had used Celsius temperatures, you would have predicted that the pressure should double, which is far greater than the actual increase. Part B Previous Answers Nitrogen gas is introduced into a large deflated plastic bag. No gas is allowed to escape, but as more and more nitrogen is added, the bag inflates to accommodate it. The pressure of the gas within the bag remains at 1.00 atm and its temperature remains at room temperature (20.0°C). How many moles 12 have been introduced into the bag by the time its volume reaches 22.4 L? Express your answer in moles. ▸ View Available Hint(s) TL = Templates Symbols undo' rego reset keyboard shortcuts help 2/ Submit mol
Transcribed Image Text:Learning Goal: To understand the ideal gas law and be able to apply it to a wide variety of situations. The absolute temperature T, volume V, and pressure P of a gas sample are related by the ideal gas law, which states that pV=nRT. Here is the number of moles in the gas sample and R is a gas constant that applies to all gases. This empirical law describes gases well only if they are sufficiently dilute and at a sufficiently high temperature that they are not on the verge of condensing. In applying the ideal gas law, p must be the absolute pressure, measured with respect to vacuum and not with respect to atmospheric pressure, and T must be the absolute temperature, measured in kelvins (that is, with respect to absolute zero, defined throughout this tutorial as -273°C). If p is in pascals and V is in cubic meters, use R = 8.3145 J/(mol-K). If p is in atmospheres and V is in liters, use R 0.08206 L atm/(mol-K) instead. A gas sample enclosed in a rigid metal container at room temperature (20.0°C) has an absolute pressure pi. The container is immersed in hot water until it warms to 40.0°C. What is the new absolute pressure p2? Express your answer in terms of p₁. ▸ View Available Hint(s) P2 = 1.07p1 Submit ✓ Correct This modest temperature increase (in absolute terms) leads to a pressure increase of just a few percent. Note that it is critical for the temperatures to be converted to absolute units. If you had used Celsius temperatures, you would have predicted that the pressure should double, which is far greater than the actual increase. Part B Previous Answers Nitrogen gas is introduced into a large deflated plastic bag. No gas is allowed to escape, but as more and more nitrogen is added, the bag inflates to accommodate it. The pressure of the gas within the bag remains at 1.00 atm and its temperature remains at room temperature (20.0°C). How many moles 12 have been introduced into the bag by the time its volume reaches 22.4 L? Express your answer in moles. ▸ View Available Hint(s) TL = Templates Symbols undo' rego reset keyboard shortcuts help 2/ Submit mol
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