In the laboratory a student determines the specific heat of a metal. He heats 18.4 grams of platinum to 99.28 °C and then drops it into an insulated cup containing 85.3 grams of water at 23.56 °C. When thermal equilibrium is reached, he measures the final temperature to be 24.10 °C. Assuming that all of the heat is transferred to the water, he calculates the specific heat of platinum to be J/g°C.
In the laboratory a student determines the specific heat of a metal. He heats 18.4 grams of platinum to 99.28 °C and then drops it into an insulated cup containing 85.3 grams of water at 23.56 °C. When thermal equilibrium is reached, he measures the final temperature to be 24.10 °C. Assuming that all of the heat is transferred to the water, he calculates the specific heat of platinum to be J/g°C.
Chemistry
10th Edition
ISBN:9781305957404
Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Chapter6: Thermochemistry
Section: Chapter Questions
Problem 64E: A 110.-g sample of copper (specific heat capacity = 0.20 J/C g) is heated to 82.4C and then placed...
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In the laboratory a student determines the specific heat of a metal.
He heats 18.4 grams of platinum to 99.28 °C and then drops it into an insulated cup containing 85.3 grams of water at 23.56 °C. When thermal equilibrium is reached, he measures the final temperature to be 24.10 °C.
Assuming that all of the heat is transferred to the water, he calculates the specific heat of platinum to be J/g°C.
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