12. A 5.00-g sample of aluminum pellets (CAI 0.89 J/(g °C)) and a 10.00-g sample of iron pellets (CFe = 0.45 J/(g °C)) are heated to 100.0 °C. The mixture of hot iron and aluminum is then dropped into 97.3 g of water at 22.0 °C. Calculate the final temperature of the metal and water mixture, assuming no heat lost to the surroundings. %3D %3D Heat released by iron and aluminum pellets = Heat absorbed by water %3D 0 = qAi + qFe + qwater = MAICAIATAI + mFeCFeATFe+ mwaterCwaterATwater Good luck with the Algebra on this one!!!!! I suggest using the solver function on your calculator instead. Using a calculator, Tr = 23.7 °C

12. A 5.00-g sample of aluminum pellets (CAI 0.89 J/(g °C)) and a 10.00-g sample of iron pellets (CFe = 0.45 J/(g °C)) are heated to 100.0 °C. The mixture of hot iron and aluminum is then dropped into 97.3 g of water at 22.0 °C. Calculate the final temperature of the metal and water mixture, assuming no heat lost to the surroundings. %3D %3D Heat released by iron and aluminum pellets = Heat absorbed by water %3D 0 = qAi + qFe + qwater = MAICAIATAI + mFeCFeATFe+ mwaterCwaterATwater Good luck with the Algebra on this one!!!!! I suggest using the solver function on your calculator instead. Using a calculator, Tr = 23.7 °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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