2. An 88.5 gram piece of iron initially at 78.8°C is place in a beaker containing 244 grams of water at 18.8°C. When thermal equilibrium is reached, what is the final temperature? The specific heat capacity for iron is 0.449 J/(g.°C). Assume no heat loss to the surroundings. Assume no heat lost to the surroundings: Heat released by the metal = Heat absorbed by water %3D -qmetal = qwater > qmetal + qwater = 0 %3D mmetalCmetalATmetal + mwaterCwaterATwater = TF = 21.0 °C
2. An 88.5 gram piece of iron initially at 78.8°C is place in a beaker containing 244 grams of water at 18.8°C. When thermal equilibrium is reached, what is the final temperature? The specific heat capacity for iron is 0.449 J/(g.°C). Assume no heat loss to the surroundings. Assume no heat lost to the surroundings: Heat released by the metal = Heat absorbed by water %3D -qmetal = qwater > qmetal + qwater = 0 %3D mmetalCmetalATmetal + mwaterCwaterATwater = TF = 21.0 °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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![2. An 88.5 gram piece of iron initially at 78.8°C is place in a beaker containing 244 grams of
water at 18.8°C. When thermal equilibrium is reached, what is the final temperature? The
specific heat capacity for iron is 0.449 J/(g·°C). Assume no heat loss to the surroundings.
Assume no heat lost to the surroundings: Heat released by the metal = Heat absorbed by water
%3D
→ qmetal + qwater = 0
%3|
-qmetal = qwater
%3D
mmetalCmetalATmetal + mwaterCwaterATwater = 0
TF = 21.0 °C
%3D](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2F61b75115-d70f-4fe2-af93-2076876ad69a%2Fd164dd58-3108-4b9f-8c42-cdbe82dd3939%2Fknv3xlg_processed.jpeg&w=3840&q=75)
Transcribed Image Text:2. An 88.5 gram piece of iron initially at 78.8°C is place in a beaker containing 244 grams of
water at 18.8°C. When thermal equilibrium is reached, what is the final temperature? The
specific heat capacity for iron is 0.449 J/(g·°C). Assume no heat loss to the surroundings.
Assume no heat lost to the surroundings: Heat released by the metal = Heat absorbed by water
%3D
→ qmetal + qwater = 0
%3|
-qmetal = qwater
%3D
mmetalCmetalATmetal + mwaterCwaterATwater = 0
TF = 21.0 °C
%3D
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