A calorimeter contains 510 mL of water at 21.5oC. A 323 g piece of iron is heated in a Bunsen burner flame, then quickly submerged in the water in the calorimeter. After adding the hot iron, the temperature of the water in the calorimeter rises to a maximum of 37.7oC. Determine the temperature (in oC) to which the piece of iron was heated. Use the following values for your calculations. specific heat of water: 4.184 J/goC density of water: 1.0 g/mL specific heat of iron: 0.449 J/goC oC
A calorimeter contains 510 mL of water at 21.5oC. A 323 g piece of iron is heated in a Bunsen burner flame, then quickly submerged in the water in the calorimeter. After adding the hot iron, the temperature of the water in the calorimeter rises to a maximum of 37.7oC. Determine the temperature (in oC) to which the piece of iron was heated. Use the following values for your calculations. specific heat of water: 4.184 J/goC density of water: 1.0 g/mL specific heat of iron: 0.449 J/goC oC
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
Chapter1: Chemical Foundations
Section: Chapter Questions
Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...
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A calorimeter contains 510 mL of water at 21.5oC. A 323 g piece of iron is heated in a Bunsen burner flame, then quickly submerged in the water in the calorimeter. After adding the hot iron, the temperature of the water in the calorimeter rises to a maximum of 37.7oC. Determine the temperature (in oC) to which the piece of iron was heated.
Use the following values for your calculations.
specific heat of water: 4.184 J/goC
density of water: 1.0 g/mL
specific heat of iron: 0.449 J/goC
oC
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