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A piece of metal weighing 59.0 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) In a coffee-cup calorimeter, 100.0 g of H20 and 100.0 mL of HCl are mixed. The HCI had an initial temperature of 44.6 oC and the water was originally at 24.6 oC. After the reaction, the temperature of both substances is 31.3 oC. a.Was the reaction exothermic or endothermic? Explain. b. Calculate how much heat the water lost or gained.

A piece of metal weighing 59.0 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) In a coffee-cup calorimeter, 100.0 g of H20 and 100.0 mL of HCl are mixed. The HCI had an initial temperature of 44.6 oC and the water was originally at 24.6 oC. After the reaction, the temperature of both substances is 31.3 oC. a.Was the reaction exothermic or endothermic? Explain. b. Calculate how much heat the water lost or gained.

Chemistry: Principles and Reactions
Chemistry: Principles and Reactions
8th Edition
ISBN:9781305079373
Author:William L. Masterton, Cecile N. Hurley
Publisher:William L. Masterton, Cecile N. Hurley
Chapter8: Thermochemistry
Section: Chapter Questions
Problem 80QAP: Equal masses of liquid A, initially at 100C, and liquid B, initially at 50C, are combined in an...
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A piece of metal weighing 59.0 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)
Transcribed Image Text:A piece of metal weighing 59.0 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)
In a coffee-cup calorimeter, 100.0 g of H20 and 100.0 mL of HCl are mixed. The HCI had an initial temperature of 44.6 oC and the water was originally at 24.6 oC. After the reaction, the temperature of both substances is 31.3 oC. a.Was the reaction exothermic or endothermic? Explain. b. Calculate how much heat the water lost or gained.
Transcribed Image Text:In a coffee-cup calorimeter, 100.0 g of H20 and 100.0 mL of HCl are mixed. The HCI had an initial temperature of 44.6 oC and the water was originally at 24.6 oC. After the reaction, the temperature of both substances is 31.3 oC. a.Was the reaction exothermic or endothermic? Explain. b. Calculate how much heat the water lost or gained.
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