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8. 98.3 J of heat is supplied to 12.28 g of a substance, and its temperature rises by 5.42C. What is the specific heat of the substance? 9. 755 J of heat is supplied to 34.0 g of water, and a additional 755 J of heat is supplied to 34.0 g of iron. If both samples are originally at 20.0°C, calculate the final temperature of the water and the iron. Comment on the difference in your answers, and explain why water is used as a coolant in a car radiator.

8. 98.3 J of heat is supplied to 12.28 g of a substance, and its temperature rises by 5.42C. What is the specific heat of the substance? 9. 755 J of heat is supplied to 34.0 g of water, and a additional 755 J of heat is supplied to 34.0 g of iron. If both samples are originally at 20.0°C, calculate the final temperature of the water and the iron. Comment on the difference in your answers, and explain why water is used as a coolant in a car radiator.

Introduction to Chemical Engineering Thermodynamics
Introduction to Chemical Engineering Thermodynamics
8th Edition
ISBN:9781259696527
Author:J.M. Smith Termodinamica en ingenieria quimica, Hendrick C Van Ness, Michael Abbott, Mark Swihart
Publisher:J.M. Smith Termodinamica en ingenieria quimica, Hendrick C Van Ness, Michael Abbott, Mark Swihart
Chapter1: Introduction
Section: Chapter Questions
Problem 1.1P
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Question 8 please
1. What is one potential use for substances that have a large amount of chemical potential energy? What happens to that energy? 2. Describe what happens when two objects that have different temperatures come into contact with one another. 3. Describe the difference between an endothermic and an exothermic reaction. 4. Two different reactions are performed in two identical test tubes. In reaction A, the test tube becomes very warm as the reaction occurs. In reaction B, the test tube becomes cold. Which reaction is endothermic and which is exothermic? Explain. 5. What is the sign of q for an endothermic process? For an exothermic process? 6. Classify the following as endothermic or exothermmic processes. a. boiling water b. running a race c. buming paper d. water freezing 7. Make the following energy conversions. a. 345 cal to Cal b. 86.8 cal to J c. 217J to cal d. 1.39 x 10' cal to kJ 8. 98.3 J of heat is supplied to 12.28 g of a substance, and its temperature rises by 5.42"C. What is the specific heat of the substance? 9. 755 J of heat is supplied to 34.0 g of water, and aă additional 755 J of heat is supplied to 34.0 g of iron. If both samples are originally at 20.0°C, calculate the final temperature of the water and the iron. Comment on the difference in your answers, and explain why water is used as a coolant in a car radiator. 10. A quantity of ethanol is cooled from 47.9°C to 12.3°C and releases 3.12 kJ of heat. What is the mass of the ethanol sample? II. How much heat is absorbed as 7.56 g of ice is heated from -30.0°C to its normal melting point?
Transcribed Image Text:1. What is one potential use for substances that have a large amount of chemical potential energy? What happens to that energy? 2. Describe what happens when two objects that have different temperatures come into contact with one another. 3. Describe the difference between an endothermic and an exothermic reaction. 4. Two different reactions are performed in two identical test tubes. In reaction A, the test tube becomes very warm as the reaction occurs. In reaction B, the test tube becomes cold. Which reaction is endothermic and which is exothermic? Explain. 5. What is the sign of q for an endothermic process? For an exothermic process? 6. Classify the following as endothermic or exothermmic processes. a. boiling water b. running a race c. buming paper d. water freezing 7. Make the following energy conversions. a. 345 cal to Cal b. 86.8 cal to J c. 217J to cal d. 1.39 x 10' cal to kJ 8. 98.3 J of heat is supplied to 12.28 g of a substance, and its temperature rises by 5.42"C. What is the specific heat of the substance? 9. 755 J of heat is supplied to 34.0 g of water, and aă additional 755 J of heat is supplied to 34.0 g of iron. If both samples are originally at 20.0°C, calculate the final temperature of the water and the iron. Comment on the difference in your answers, and explain why water is used as a coolant in a car radiator. 10. A quantity of ethanol is cooled from 47.9°C to 12.3°C and releases 3.12 kJ of heat. What is the mass of the ethanol sample? II. How much heat is absorbed as 7.56 g of ice is heated from -30.0°C to its normal melting point?
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