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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
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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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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