A 15.7 g aluminum block is warmed to 53.2 deg C and plunged into an insulated beaker containing 32.5 g of water initially at 24.5 deg 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 15.7 g aluminum block is warmed to 53.2 deg C and plunged into an insulated beaker containing 32.5 g of water initially at 24.5 deg 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
Chapter6: Thermochemistry
Section: Chapter Questions
Problem 64E: A 110.-g sample of copper (specific heat capacity = 0.20 J/C g) is heated to 82.4C and then placed...
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A 15.7 g aluminum block is warmed to 53.2 deg C and plunged into an insulated beaker containing 32.5 g of water initially at 24.5 deg 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?
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