Question 6 is based on the question 2 so in case you need it NameDateAlec NemaScore12/9/2020HOMEWORK FOR LAB 4:THE FIRST LAW OF THERMODYNAMICS (RTP2-4)1. Describe what happens to the temperature of water between 0 and 100°Cwhen heat energy is transferred to it at a constant rate.When heaf energy is trans ferred to water atarate, then the time taken to raise the tempthe water at initial stage,ato°c iş higher aftime taken to raise the température of thewateri2. Describe what happens to the temperature df a water-ice mixture originallyat 0°C when heat energy is transferred to it at a constant rate. Sketch a decre9temperature history on the axes below. Indicate on your graph where the icehas completely melted,when heat trans ferred to water-jce mixturefirst temperature docsn't increase tall, until all sice has melt towater. 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 waterTme (min)temperature increasesmixture if the temperature does not rise while the ice is melting. How doesthe internal energy of the ice and water mixture change during this process?Doęs it increase, decrease, or remain the same? Explain. no externeis supplied, then the ice starts melting by absorbing heat energy from thanges Completely into water at constant temperature. Atthisof ice increases and the internal gneryy of water decreaseenevgyheat energy issupeliedand the temperature of the mixture is mainted.c4. Suppose you start with 250 g of ice at 0°C. Calculate the amount of heat suenergy that must be transferred to the ice to melt it. (Use 334 x 103 J/kg forthe latent heat of fusion of ice.) Show your calculations. and their interrthe enargy is interemass of ice =250 g=0.25 kgLatent of fusion Le= 334x103 J/kgheatamount of 'heatenergy U=m.Lp=0.25 kgxXU=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 haformotted 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 ofheat energy must be transferred to bring this mixture to a final temperature of75°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 offusion 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 saInifial temperature of ice =T,initial temperat ure of wat er TiQ1=S0100J+471het 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 totransfer heat energy at a constant rate even after the ice had melted. Sketchthe temperature history on the axes below. Indicate on your graph the timewhen the water begins to boil.100Time (min)7. Explain what happens to the heat energy transferred to the water and steammixture if the temperature does not rise while the water is boiling. How doesthe internal energy of the water and steam mixture change during thisprocess? Does it increase, decrease, or remain the same? Explain. NOw, wherenergy is supplied, then the ice starts meiting by abfrom the water. lce changes Completely intő waterAt this condition, internal energy of ice increasesenergy of water decreases.If the external energthe Femperature is maintained constant, then theis absorbed by both water and ice. Their internaland then energy is the thermel potential eneryySuppose you start with 250 g of ice at 0°C. Calculate the amount of heatTemperature (°C)

Question

Question 6 is based on the question 2 so in case you need it NameDateAlec NemaScore12/9/2020HOMEWORK FOR LAB 4:THE FIRST LAW OF THERMODYNAMICS (RTP2-4)1. Describe what happens to the temperature of water between 0 and 100°Cwhen heat energy is transferred to it at a constant rate.When heaf energy is trans ferred to water atarate, then the time taken to raise the tempthe water at initial stage,ato°c iş higher aftime taken to raise the température of thewateri2. Describe what happens to the temperature df a water-ice mixture originallyat 0°C when heat energy is transferred to it at a constant rate. Sketch a decre9temperature history on the axes below. Indicate on your graph where the icehas completely melted,when heat trans ferred to water-jce mixturefirst temperature docsn't increase tall, until all sice has melt towater. 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 waterTme (min)temperature increasesmixture if the temperature does not rise while the ice is melting. How doesthe internal energy of the ice and water mixture change during this process?Doęs it increase, decrease, or remain the same? Explain. no externeis supplied, then the ice starts melting by absorbing heat energy from thanges Completely into water at constant temperature. Atthisof ice increases and the internal gneryy of water decreaseenevgyheat energy issupeliedand the temperature of the mixture is mainted.c4. Suppose you start with 250 g of ice at 0°C. Calculate the amount of heat suenergy that must be transferred to the ice to melt it. (Use 334 x 103 J/kg forthe latent heat of fusion of ice.) Show your calculations. and their interrthe enargy is interemass of ice =250 g=0.25 kgLatent of fusion Le= 334x103 J/kgheatamount of 'heatenergy U=m.Lp=0.25 kgxXU=8. 35 x10&#34;J=83.5 KJ)Written by David R. Sokoloff, Ronald Thornton, and Priscilla Laws 1999 John Wiley & Sons. Portions of this material haformotted 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 ofheat energy must be transferred to bring this mixture to a final temperature of75°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 offusion 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 saInifial temperature of ice =T,initial temperat ure of wat er TiQ1=S0100J+471het 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 totransfer heat energy at a constant rate even after the ice had melted. Sketchthe temperature history on the axes below. Indicate on your graph the timewhen the water begins to boil.100Time (min)7. Explain what happens to the heat energy transferred to the water and steammixture if the temperature does not rise while the water is boiling. How doesthe internal energy of the water and steam mixture change during thisprocess? Does it increase, decrease, or remain the same? Explain. NOw, wherenergy is supplied, then the ice starts meiting by abfrom the water. lce changes Completely intő waterAt this condition, internal energy of ice increasesenergy of water decreases.If the external energthe Femperature is maintained constant, then theis absorbed by both water and ice. Their internaland then energy is the thermel potential eneryySuppose you start with 250 g of ice at 0°C. Calculate the amount of heatTemperature (°C)

Accepted Answer

When heat energy is transferred to ice at temperature 0° C , this heat energy will be used for the…