A 47.0-g sample of copper at 99.9 °C is dropped into a beaker containing 157 g of water at 19.0 °C. What is the final temperature when thermal equilibrium is reached? (The specific heat capacities of liquid water and copper are 4.184 J/g K and 0.385 J/g K, respectively.)

A 47.0-g sample of copper at 99.9 °C is dropped into a beaker containing 157 g of water at 19.0 °C. What is the final temperature when thermal equilibrium is reached? (The specific heat capacities of liquid water and copper are 4.184 J/g K and 0.385 J/g K, respectively.)

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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Question

A 47.0-g sample of copper at 99.9 °C is dropped into a beaker containing 157 g of water at 19.0 °C. What is the final temperature when thermal equilibrium is reached? (The specific
heat capacities of liquid water and copper are 4.184 J/g K and 0.385 J/g K, respectively.)
Final temperature =
°C
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