When 2.1 kg of water at 12.3 °C is mixed with 3.7 kg of water at 39.7 °C in a well-insulated container, what is the change in entropy of the system?
When 2.1 kg of water at 12.3 °C is mixed with 3.7 kg of water at 39.7 °C in a well-insulated container, what is the change in entropy of the system?
Chapter4: The Second Law Of Thermodynamics
Section: Chapter Questions
Problem 51P: One mole of an ideal monatomic gas is confined to a rigid container. When heat is added reversibly...
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![When 2.1 kg of water at 12.3 °C is mixed with 3.7 kg of water at 39.7
°C in a well-insulated container, what is the change in entropy of the
system?
Part A
Make an estimate.
Express your answer to two significant figures and include the appropriate units.
HÁ
?
AS =
Value
Units
Submit
Request Answer
Part B
Use the integral AS = [dQ/T.
Express your answer to two significant figures and include the appropriate units.
HA
AS =
Value
Units
Submit
Request Answer](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2Fe7978552-0588-4e79-b0df-6edbc7f1b95a%2Fd5b08489-8982-4f34-8068-ed6ed9ca9604%2Farublm_processed.png&w=3840&q=75)
Transcribed Image Text:When 2.1 kg of water at 12.3 °C is mixed with 3.7 kg of water at 39.7
°C in a well-insulated container, what is the change in entropy of the
system?
Part A
Make an estimate.
Express your answer to two significant figures and include the appropriate units.
HÁ
?
AS =
Value
Units
Submit
Request Answer
Part B
Use the integral AS = [dQ/T.
Express your answer to two significant figures and include the appropriate units.
HA
AS =
Value
Units
Submit
Request Answer
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