18. Two different metals, lead and copper, are heated to 100°C and each is immersed into a separate calorimeter containing 50.0 g of water at 20°C. The experimenter observed that 3.0 g of lead produced the same final temperature as 1.0g of copper. Which statement follows from this observation? a. Lead has a three times the specific heat capacity of copper. b. Copper has a three times the specific heat capacity of lead. c. Copper and lead have the same specific heat capacity. d. The final temperature does not depend on the mass of the metal used.

18. Two different metals, lead and copper, are heated to 100°C and each is immersed into a separate calorimeter containing 50.0 g of water at 20°C. The experimenter observed that 3.0 g of lead produced the same final temperature as 1.0g of copper. Which statement follows from this observation? a. Lead has a three times the specific heat capacity of copper. b. Copper has a three times the specific heat capacity of lead. c. Copper and lead have the same specific heat capacity. d. The final temperature does not depend on the mass of the metal used.

Chemistry: An Atoms First Approach

2nd Edition

ISBN:9781305079243

Author:Steven S. Zumdahl, Susan A. Zumdahl

Publisher:Steven S. Zumdahl, Susan A. Zumdahl

Chapter7: Chemical Energy

Section: Chapter Questions

Problem 109AE: A sample of nickel is heated to 99.8C and placed in a coffee-cup calorimeter containing 150.0 g...

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A 500.0-g sample of an element at 195C is dropped into an ice--water mixture; 109.5 g ice melts and an ice--water mixture remains. Calculate the specific heat of the element. See Exercise 131 for pertinent information.
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9.104 An engineer is using sodium metal as a cooling agent in a design because it has useful thermal properties. Looting up the heat capacity, the engineer finds a value of 28.2 J mol-l °C-l. Carelessly, he wrote this number down without units. As a result, it was later taken as specific heat. (a) What would he the difference between these two values? (b) Would the engineer overestimate the ability of sodium to remove heat from the system or underestimate it because of this error? Be sure to explain your reasoning.
A 110.-g sample of copper (specific heat capacity = 0.20 J/C g) is heated to 82.4C and then placed in a container of water at 22.3C. The final temperature of the water and copper is 24.9C. What is the mass of the water in the container, assuming that all the heat lost by the copper is gained by the water?
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