6. A 40.00 g sample of water at 22.00°C is put in a calorimeter. After 60.00g of water at 65.00°C is added to the calorimeter, the mixture is stirred,and the final temperature is 47.00°C. Calculate the heat capacity of thecalorimeter in calfC.7. A piece of metal weighing 7.00 g is heated to 93.0°C and placed into thecalorimeter described in the previous problem. The calorimeter contains 25.0g of water at 30.0°C. If the final temperature of the water is 33.0°C, cal-culate the specific heat of the metal in cal/g °C.

(6) Given - Mass of water at 22.00°C = 40.00 g Mass of water at 65.00°C = 60.00 g Final…

6. A 40.00 g sample of water at 22.00°C is put in a calorimeter. After 60.00 g of water at 65.00°C is added to the calorimeter, the mixture is stirred, and the final temperature is 47.00°C. Calculate the heat capacity of th. calorimeter in calPC. 7. A piece of metal weighing 7.00 g is heated to 93.0°C and placed into the calorimeter described in the previous problem. The calorimeter contains 25. g of water at 30.0°C. If the final temperature of the water is 33.0°C, cal- ifin hoot off the metal in cal/g °C. 0uloto

6. A 40.00 g sample of water at 22.00°C is put in a calorimeter. After 60.00 g of water at 65.00°C is added to the calorimeter, the mixture is stirred, and the final temperature is 47.00°C. Calculate the heat capacity of th. calorimeter in calPC. 7. A piece of metal weighing 7.00 g is heated to 93.0°C and placed into the calorimeter described in the previous problem. The calorimeter contains 25. g of water at 30.0°C. If the final temperature of the water is 33.0°C, cal- ifin hoot off the metal in cal/g °C. 0uloto

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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