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Specific Heat Capacities of common substances: Water (1) = 4.184 Iron (s) =0.45L Aluminum (s) = 0.89 L Mercury () = 0.14 Carbon (s) = 0.71 g-K Silver (s) = 0.24 - Gold (s) = 0.13L Brass (yellow solid alloy) = 0.402 - A piece of metal weighing 59.047 g was heated to 100.0°C and then put it into 100.0 mL of water (initially at 23.7°C). The metal and water were allowed to come to an equilibrium temperature, determined to be 27.8°C. Assuming no heat lost to the environment, calculate the specific heat of the metal. (Hint: First calculate the heat absorbed by the water then use this value for "q" to determine the specific heat of the metal in a second calculation.) Compare your result to the above list of substances. What could the metal be?

Specific Heat Capacities of common substances: Water (1) = 4.184 Iron (s) =0.45L Aluminum (s) = 0.89 L Mercury () = 0.14 Carbon (s) = 0.71 g-K Silver (s) = 0.24 - Gold (s) = 0.13L Brass (yellow solid alloy) = 0.402 - A piece of metal weighing 59.047 g was heated to 100.0°C and then put it into 100.0 mL of water (initially at 23.7°C). The metal and water were allowed to come to an equilibrium temperature, determined to be 27.8°C. Assuming no heat lost to the environment, calculate the specific heat of the metal. (Hint: First calculate the heat absorbed by the water then use this value for "q" to determine the specific heat of the metal in a second calculation.) Compare your result to the above list of substances. What could the metal be?

General Chemistry - Standalone book (MindTap Course List)
General Chemistry - Standalone book (MindTap Course List)
11th Edition
ISBN:9781305580343
Author:Steven D. Gammon, Ebbing, Darrell Ebbing, Steven D., Darrell; Gammon, Darrell Ebbing; Steven D. Gammon, Darrell D.; Gammon, Ebbing; Steven D. Gammon; Darrell
Publisher:Steven D. Gammon, Ebbing, Darrell Ebbing, Steven D., Darrell; Gammon, Darrell Ebbing; Steven D. Gammon, Darrell D.; Gammon, Ebbing; Steven D. Gammon; Darrell
Chapter6: Thermochemisty
Section: Chapter Questions
Problem 6.144QP: A piece of iron was heated to 95.4C and dropped into a constant-pressure calorimeter containing 284...
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Specific Heat Capacities of common substances: Water () = 4.184- Iron (s) - 0.45 Aluminum (s) = 0.89 - g-K Mercury (I) = 0.14- Carbon (s) = 0.71- Silver (s) = 0.24 g-K Gold (s) = 0.13 Brass (yellow solid alloy) = 0.402 - A piece of metal weighing 59.047 g was heated to 100.0°C and then put it into 100.0 mL of water (initially at 23.7°C). The metal and water were allowed to come to an equilibrium temperature, determined to be 27.8°C. Assuming no heat lost to the environment, calculate the specific heat of the metal. (Hint: First calculate the heat absorbed by the water then use this value for “q" to determine the specific heat of the metal in a second calculation.) Compare your result to the above list of substances. What could the metal be?
Transcribed Image Text:Specific Heat Capacities of common substances: Water () = 4.184- Iron (s) - 0.45 Aluminum (s) = 0.89 - g-K Mercury (I) = 0.14- Carbon (s) = 0.71- Silver (s) = 0.24 g-K Gold (s) = 0.13 Brass (yellow solid alloy) = 0.402 - A piece of metal weighing 59.047 g was heated to 100.0°C and then put it into 100.0 mL of water (initially at 23.7°C). The metal and water were allowed to come to an equilibrium temperature, determined to be 27.8°C. Assuming no heat lost to the environment, calculate the specific heat of the metal. (Hint: First calculate the heat absorbed by the water then use this value for “q" to determine the specific heat of the metal in a second calculation.) Compare your result to the above list of substances. What could the metal be?
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