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to bring water=M2XC2X(1-T,)Q Describe what would happef to the water in Question 2 if you continued to transfer heat energy at a constant rate even after the ice had melted. Sketch the temperature history on the axes below. Indicate on your graph the time when the water begins to boil. 100 Time (min) Temperature (°C)

to bring water=M2XC2X(1-T,)Q Describe what would happef to the water in Question 2 if you continued to transfer heat energy at a constant rate even after the ice had melted. Sketch the temperature history on the axes below. Indicate on your graph the time when the water begins to boil. 100 Time (min) Temperature (°C)

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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Question 6 is based on the question 2 so in case you need it
Name Date Alec Nema Score 12/9/2020 HOMEWORK FOR LAB 4: THE FIRST LAW OF THERMODYNAMICS (RTP2-4) 1. Describe what happens to the temperature of water between 0 and 100°C when heat energy is transferred to it at a constant rate. When heaf energy is trans ferred to water ata rate, then the time taken to raise the temp the water at initial stage,ato°c iş higher af time taken to raise the température of thewateri 2. Describe what happens to the temperature df a water-ice mixture originally at 0°C when heat energy is transferred to it at a constant rate. Sketch a decre9 temperature history on the axes below. Indicate on your graph where the ice has completely melted, when heat trans ferred to water-jce mixture first temperature docsn't increase t all, until all sice has melt to water. Once jce converts to water, then temperature rises upto 100° Then, again it changes to vapos- atlo0°C, and then aganng tolain what happens to the heat energy transferred to the ice and water Tme (min) temperature increases mixture if the temperature does not rise while the ice is melting. How does the internal energy of the ice and water mixture change during this process? Doęs it increase, decrease, or remain the same? Explain. no externe is supplied, then the ice starts melting by absorbing heat energy from t hanges Completely into water at constant temperature. Atthis of ice increases and the internal gneryy of water decrease enevgy heat energy issupeliedand the temperature of the mixture is mainted.c 4. Suppose you start with 250 g of ice at 0°C. Calculate the amount of heat su energy that must be transferred to the ice to melt it. (Use 334 x 103 J/kg for the latent heat of fusion of ice.) Show your calculations. and their interr the enargy is intere mass of ice =250 g=0.25 kg Latent of fusion Le= 334x103 J/kg heat amount of 'heat energy U=m.Lp=0.25 kgxX U=8. 35 x10"J=83.5 KJ) Written by David R. Sokoloff, Ronald Thornton, and Priscilla Laws 1999 John Wiley & Sons. Portions of this material ha formotted hy W Duxler (2/8/2004); A. Kocharian (02/24/2006) with assistance from R. Pelka; M. Wesslin
Transcribed Image Text:Name Date Alec Nema Score 12/9/2020 HOMEWORK FOR LAB 4: THE FIRST LAW OF THERMODYNAMICS (RTP2-4) 1. Describe what happens to the temperature of water between 0 and 100°C when heat energy is transferred to it at a constant rate. When heaf energy is trans ferred to water ata rate, then the time taken to raise the temp the water at initial stage,ato°c iş higher af time taken to raise the température of thewateri 2. Describe what happens to the temperature df a water-ice mixture originally at 0°C when heat energy is transferred to it at a constant rate. Sketch a decre9 temperature history on the axes below. Indicate on your graph where the ice has completely melted, when heat trans ferred to water-jce mixture first temperature docsn't increase t all, until all sice has melt to water. Once jce converts to water, then temperature rises upto 100° Then, again it changes to vapos- atlo0°C, and then aganng tolain what happens to the heat energy transferred to the ice and water Tme (min) temperature increases mixture if the temperature does not rise while the ice is melting. How does the internal energy of the ice and water mixture change during this process? Doęs it increase, decrease, or remain the same? Explain. no externe is supplied, then the ice starts melting by absorbing heat energy from t hanges Completely into water at constant temperature. Atthis of ice increases and the internal gneryy of water decrease enevgy heat energy issupeliedand the temperature of the mixture is mainted.c 4. Suppose you start with 250 g of ice at 0°C. Calculate the amount of heat su energy that must be transferred to the ice to melt it. (Use 334 x 103 J/kg for the latent heat of fusion of ice.) Show your calculations. and their interr the enargy is intere mass of ice =250 g=0.25 kg Latent of fusion Le= 334x103 J/kg heat amount of 'heat energy U=m.Lp=0.25 kgxX U=8. 35 x10"J=83.5 KJ) Written by David R. Sokoloff, Ronald Thornton, and Priscilla Laws 1999 John Wiley & Sons. Portions of this material ha formotted hy W Duxler (2/8/2004); A. Kocharian (02/24/2006) with assistance from R. Pelka; M. Wesslin
5. A mixture of 150 g of ice and 300 a of water is at 0°C. How many joules of heat energy must be transferred to bring this mixture to a final temperature of 75°C? Assume that the heat energy transferred to the room is very small. Show your calculations. [Use 334 x 103 J/kg (334 J/g) for the latent heat of fusion of ice and 4190 J/kg°C (4.19 J/g°C) for the specific heat of water.] Final temperature =75°C =T heat required to be sa Inifial temperature of ice =T, initial temperat ure of wat er Ti Q1=S0100J+471 het required= mixL tm c (T+Fi)=Q2=91275,. heat required to bring water=m2 XC2X(T-T,)=Q2 Q. 6. Describe what would happeR to the water in Question 2 if you continued to transfer heat energy at a constant rate even after the ice had melted. Sketch the temperature history on the axes below. Indicate on your graph the time when the water begins to boil. 100 Time (min) 7. Explain what happens to the heat energy transferred to the water and steam mixture if the temperature does not rise while the water is boiling. How does the internal energy of the water and steam mixture change during this process? Does it increase, decrease, or remain the same? Explain. NOw, wher energy is supplied, then the ice starts meiting by ab from the water. lce changes Completely intő water At this condition, internal energy of ice increases energy of water decreases.If the external energ the Femperature is maintained constant, then the is absorbed by both water and ice. Their internal and then energy is the thermel potential eneryy Suppose you start with 250 g of ice at 0°C. Calculate the amount of heat Temperature (°C)
Transcribed Image Text:5. A mixture of 150 g of ice and 300 a of water is at 0°C. How many joules of heat energy must be transferred to bring this mixture to a final temperature of 75°C? Assume that the heat energy transferred to the room is very small. Show your calculations. [Use 334 x 103 J/kg (334 J/g) for the latent heat of fusion of ice and 4190 J/kg°C (4.19 J/g°C) for the specific heat of water.] Final temperature =75°C =T heat required to be sa Inifial temperature of ice =T, initial temperat ure of wat er Ti Q1=S0100J+471 het required= mixL tm c (T+Fi)=Q2=91275,. heat required to bring water=m2 XC2X(T-T,)=Q2 Q. 6. Describe what would happeR to the water in Question 2 if you continued to transfer heat energy at a constant rate even after the ice had melted. Sketch the temperature history on the axes below. Indicate on your graph the time when the water begins to boil. 100 Time (min) 7. Explain what happens to the heat energy transferred to the water and steam mixture if the temperature does not rise while the water is boiling. How does the internal energy of the water and steam mixture change during this process? Does it increase, decrease, or remain the same? Explain. NOw, wher energy is supplied, then the ice starts meiting by ab from the water. lce changes Completely intő water At this condition, internal energy of ice increases energy of water decreases.If the external energ the Femperature is maintained constant, then the is absorbed by both water and ice. Their internal and then energy is the thermel potential eneryy Suppose you start with 250 g of ice at 0°C. Calculate the amount of heat Temperature (°C)
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