A 7.50-g piece of iron at 100.0°C is dropped into 25.0 g of water at 22.0°C. Assuming that the heat lost by the iron equals the heat gained by the water, determine the final temperature of the iron/water system. Assume a heat capacity of water at 4.18 J/g K and of iron at 0.452 J/g K.
A 7.50-g piece of iron at 100.0°C is dropped into 25.0 g of water at 22.0°C. Assuming that the heat lost by the iron equals the heat gained by the water, determine the final temperature of the iron/water system. Assume a heat capacity of water at 4.18 J/g K and of iron at 0.452 J/g K.
Physical Chemistry
2nd Edition
ISBN:9781133958437
Author:Ball, David W. (david Warren), BAER, Tomas
Publisher:Ball, David W. (david Warren), BAER, Tomas
Chapter2: The First Law Of Thermodynamics
Section: Chapter Questions
Problem 2.15E: A7.50-gpiece of iron at 100.0C is dropped into 25.0g of water at 22.0C. Assuming that the heat lost...
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A 7.50-g piece of iron at 100.0°C is dropped into 25.0 g of water at 22.0°C. Assuming that the heat lost by the iron equals the heat gained by the water, determine the final temperature of the iron/water system. Assume a heat capacity of water at 4.18 J/g K and of iron at 0.452 J/g K.
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