2.A 102.8 g sample of a metal initially at 183.0°C is placed in 35.0 ml of water initially at 25.0 °C. After reaching thermal equilibrium, the final temperature of the system is 58.8°C. What is the identity of the metal? Assume no heat is lost to the surroundings. 58.8°C-2s.0°C= 33,8°C 25.c 358,80C Q= 0= (muoter)(water)l 3. Calculate the final temperature of the water after 2.47 g of zinc at 60.1 °C is added to 29.4 g of water at 16.4 °C. Assume no heat is lost to the surroundings.
2.A 102.8 g sample of a metal initially at 183.0°C is placed in 35.0 ml of water initially at 25.0 °C. After reaching thermal equilibrium, the final temperature of the system is 58.8°C. What is the identity of the metal? Assume no heat is lost to the surroundings. 58.8°C-2s.0°C= 33,8°C 25.c 358,80C Q= 0= (muoter)(water)l 3. Calculate the final temperature of the water after 2.47 g of zinc at 60.1 °C is added to 29.4 g of water at 16.4 °C. Assume no heat is lost to the surroundings.
Chemistry: An Atoms First Approach
2nd Edition
ISBN:9781305079243
Author:Steven S. Zumdahl, Susan A. Zumdahl
Publisher:Steven S. Zumdahl, Susan A. Zumdahl
Chapter7: Chemical Energy
Section: Chapter Questions
Problem 109AE: A sample of nickel is heated to 99.8C and placed in a coffee-cup calorimeter containing 150.0 g...
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A 102.8g sample of a metal initially at 183.0 C is placed in 35.0 ml of water initially at 25.0 C. After reaching thermal equilibrium, the final temperature of the system is 58.8 C. What is the identity of the metal? Assume no heat is lost to the surroundings.
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