A calorimeter contains 704 mL of water at 24.8°C. A 346 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 41.8°C. Determine the temperature (in °C) to which the piece of iron was heated. Use the following values for your calculations. specific heat of water: 4.184 J/g°C density of water: 1.0 g/mL specific heat of iron: 0.449 J/g°C °C

A calorimeter contains 704 mL of water at 24.8°C. A 346 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 41.8°C. Determine the temperature (in °C) to which the piece of iron was heated. Use the following values for your calculations. specific heat of water: 4.184 J/g°C density of water: 1.0 g/mL specific heat of iron: 0.449 J/g°C °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

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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