A 27.0 - g aluminum block is warmed to 65.6 °C and plunged into an insulated beaker containing 55.5 g water initially at 22.2 °C. The aluminum and the water are allowed to come to thermal equilibrium. Assuming that no heat is lost, what is the final temperature of the water and aluminum?
A 27.0 - g aluminum block is warmed to 65.6 °C and plunged into an insulated beaker containing 55.5 g water initially at 22.2 °C. The aluminum and the water are allowed to come to thermal equilibrium. Assuming that no heat is lost, what is the final temperature of the water and aluminum?
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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Step 1: Explaining the problem statement
Answer:
This problem is based on law of conservation of energy where heat lost by Al will be equal to heat gained by water because energy can't be destroyed.
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