Textbook Question
30 g of copper pellets are removed from a 300°C oven and immediately dropped into 100 mL of water at 20°C in an insulated cup. What will the new water temperature be?
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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
- Ch 29: The Magnetic Field47
- Ch 30: Electromagnetic Induction60
- Ch 31: Electromagnetic Fields and Waves32
- Ch 32: AC Circuits63
- Ch 33: Wave Optics32
- 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 24
Knight Calc 5th EditionCh 19: Work, Heat, and the First Law of ThermodynamicsProblem 24Chapter 19, Problem 24
A 65 cm3 block of iron is removed from an 800°C furnace and immediately dropped into 200 mL of 20°C water. What fraction of the water boils away?
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Convert the given volumes into masses. For the iron block, use the density of iron (approximately 7.87 g/cm³) to calculate its mass. For water, use the density of water (1 g/mL) to determine its mass.
Calculate the heat lost by the iron block as it cools from 800°C to 100°C (the boiling point of water). Use the formula for heat transfer: , where is the mass of the iron, is the specific heat capacity of iron (approximately 0.45 J/g°C), and is the temperature change.
Determine the heat required to raise the water from 20°C to 100°C using the same heat transfer formula: , where is the specific heat capacity of water (4.18 J/g°C).
Calculate the heat required to boil the water at 100°C using the formula: , where is the latent heat of vaporization of water (2260 J/g).
Compare the heat lost by the iron block to the total heat required to raise the water to 100°C and boil it. The fraction of water that boils away is the ratio of the heat available for vaporization to the heat required for vaporizing the entire mass of water.
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Key Concepts
Here are the essential concepts you must grasp in order to answer the question correctly.
Heat Transfer
Heat transfer is the process by which thermal energy moves from one object to another due to a temperature difference. In this scenario, the hot iron block will transfer heat to the cooler water until thermal equilibrium is reached. Understanding the mechanisms of conduction, convection, and radiation is essential for analyzing how heat moves between the iron and water.
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Overview of Heat Transfer
Specific Heat Capacity
Specific heat capacity is the amount of heat required to raise the temperature of a unit mass of a substance by one degree Celsius. Each material has a unique specific heat capacity, which influences how much heat it can absorb or release. In this problem, knowing the specific heat capacities of both iron and water is crucial for calculating the temperature change and the resulting heat transfer.
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Phase Change and Latent Heat
Phase change refers to the transition of a substance from one state of matter to another, such as from liquid to gas. During this process, energy is absorbed or released without a change in temperature, known as latent heat. In this question, understanding the latent heat of vaporization for water is vital to determine how much water can boil away as it absorbs heat from the iron block.
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Related Practice
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Textbook Question
An experiment measures the temperature of a 500 g substance while steadily supplying heat to it. FIGURE EX19.20 shows the results of the experiment. What are the heats of fusion and vaporization?
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Textbook Question
A monatomic gas follows the process 1→2→3 shown in FIGURE EX19.26. How much heat is needed for (a) process 1→2 and (b) process 2→3?
Textbook Question
A 750 g aluminum pan is removed from the stove and plunged into a sink filled with 10.0 L of water at 20.0°C . The water temperature quickly rises to 24.0°C. What was the initial temperature of the pan in °C and in °F?
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Textbook Question
10 g of steam at the boiling point are combined with 50 g of ice at the freezing point. What is the final temperature of the system?
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