Textbook Question
0.10 mol of nitrogen gas follow the two processes shown in FIGURE P19.58. How much heat is required for each?
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Ch 19: Work, Heat, and the First Law of Thermodynamics
Knight Calc5th EditionPhysics for Scientists and EngineersISBN: 9780137344796
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Table of contents
- Ch 01: Concepts of Motion35
- Ch 02: Kinematics in One Dimension75
- Ch 03: Vectors and Coordinate Systems58
- Ch 04: Kinematics in Two Dimensions60
- Ch 05: Force and Motion23
- Ch 06: Dynamics I: Motion Along a Line53
- Ch 07: Newton's Third Law27
- Ch 08: Dynamics II: Motion in a Plane52
- Ch 09: Work and Kinetic Energy56
- Ch 10: Interactions and Potential Energy50
- Ch 11: Impulse and Momentum56
- Ch 12: Rotation of a Rigid Body71
- Ch 13: Newton's Theory of Gravity52
- Ch 14: Fluids and Elasticity44
- Ch 15: Oscillations55
- Ch 16: Traveling Waves37
- Ch 17: Superposition39
- Ch 18: A Macroscopic Description of Matter53
- Ch 19: Work, Heat, and the First Law of Thermodynamics60
- Ch 20: The Micro/Macro Connection53
- Ch 21: Heat Engines and Refrigerators34
- Ch 22: Electric Charges and Forces40
- Ch 23: The Electric Field39
- Ch 24: Gauss' Law32
- Ch 25: The Electric Potential63
- Ch 26: Potential and Field57
- Ch 27: Current and Resistance42
- Ch 28: Fundamentals of Circuits39
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- Ch 34: Ray Optics57
- Ch 35: Optical Instruments30
- Ch 36: Special Relativity38
- Ch 37: The Foundations of Modern Physics25
- Ch 38: Quantization49
- Ch 39: Wave Functions and Uncertainty31
- Ch 40: One-Dimensional Quantum Mechanics35
- Ch 41: Atomic Physics18
- Ch 42: Nuclear Physics27
Knight Calc5th EditionPhysics for Scientists and EngineersISBN: 9780137344796Not the one you use?Change textbook
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Knight Calc 5th EditionCh 19: Work, Heat, and the First Law of ThermodynamicsProblem 57c
Knight Calc 5th EditionCh 19: Work, Heat, and the First Law of ThermodynamicsProblem 57cChapter 19, Problem 57c
5.0 g of nitrogen gas at 20°C and an initial pressure of 3.0 atm undergo an isobaric expansion until the volume has tripled. What is the gas pressure after the decrease?
Verified step by step guidance1
Step 1: Identify the type of thermodynamic process. The problem states that the process is isobaric, meaning the pressure remains constant throughout the expansion. Therefore, the gas pressure after the expansion will be the same as the initial pressure.
Step 2: Recall the definition of an isobaric process. In an isobaric process, the pressure does not change, so the final pressure is equal to the initial pressure. Mathematically, \( P_{final} = P_{initial} \).
Step 3: Substitute the given initial pressure into the equation. The initial pressure is \( P_{initial} = 3.0 \; \text{atm} \).
Step 4: Conclude that since the pressure remains constant during an isobaric process, the final pressure \( P_{final} \) is also \( 3.0 \; \text{atm} \).
Step 5: Note that no further calculations are needed because the pressure does not change in an isobaric process. The final pressure is directly equal to the initial pressure.
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Key Concepts
Here are the essential concepts you must grasp in order to answer the question correctly.
Isobaric Process
An isobaric process is a thermodynamic process in which the pressure remains constant while the volume and temperature of the gas may change. In this scenario, the nitrogen gas expands at a constant pressure of 3.0 atm, which means that any changes in volume will not affect the pressure until the process is complete.
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Ideal Gas Law
The Ideal Gas Law relates the pressure, volume, temperature, and number of moles of a gas through the equation PV = nRT. This law is essential for understanding the behavior of gases under various conditions, allowing us to predict how changes in volume and temperature affect pressure, especially in processes like isobaric expansion.
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Charles's Law
Charles's Law states that the volume of a gas is directly proportional to its temperature when pressure is held constant. In this case, as the nitrogen gas expands and its volume triples, the temperature will also change, which can be calculated to determine the final state of the gas after the expansion.
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Related Practice
Textbook Question
5.0 g of nitrogen gas at 20°C and an initial pressure of 3.0 atm undergo an isobaric expansion until the volume has tripled. What amount of heat energy is transferred from the gas as its pressure decreases?
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Textbook Question
5.0 g of nitrogen gas at 20°C and an initial pressure of 3.0 atm undergo an isobaric expansion until the volume has tripled. How much heat energy is transferred to the gas to cause this expansion?
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Textbook Question
Two cylinders each contain 0.10 mol of a diatomic gas at 300 K and a pressure of 3.0 atm. Cylinder A expands isothermally and cylinder B expands adiabatically until the pressure of each is 1.0 atm. What are the final temperature and volume of each?
Textbook Question
5.0 g of nitrogen gas at 20°C and an initial pressure of 3.0 atm undergo an isobaric expansion until the volume has tripled. What are the gas volume and temperature after the expansion?
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Textbook Question
n moles of an ideal gas at temperature T1 and volume V1 expand isothermally until the volume has doubled. In terms of n, T1, and V1, what are the heat energy transferred to the gas?
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