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5. Why, on exothermic time-temperature graph, does the temperature eventually fall? 6. How many kJ of energy are required to change 1.00 m3 of pure water by 1.0 °C Assume a perfect system. The specific heat of the water is 4.184 J/g °C. The density of water is 1.000 g/mL. 1.00 m3 = 1000 Litres 7. 2.500 grams of metal X (molar mass 65.39 g/mole) was reacted with 100.0 mL of a 1.500 M HCI solution in a coffee cup calorimeter. The temperature went from 12.50 °C to 40.50 °C. Determine the reaction enthalpy per mole of metal X. The specific heat of the solution is 4.184 J/g o°C. Assume a solution density of 1.00 g/mL and a perfect system. 8. 20.12 grams of butane, C4H10, was combusted with oxygen in a bomb calorimeter. The temperature of 0.500 kilograms of water went from 5.00 oC to 25.89 °C. The specific heat of the water is 4.184 J/g °C. Assume a solution density of 1.00 g/mL. Determine the heat (kJ) evolved per mole of butane. Assume a perfect bomb calorimeter. See pre-laboratory letter e.

5. Why, on exothermic time-temperature graph, does the temperature eventually fall? 6. How many kJ of energy are required to change 1.00 m3 of pure water by 1.0 °C Assume a perfect system. The specific heat of the water is 4.184 J/g °C. The density of water is 1.000 g/mL. 1.00 m3 = 1000 Litres 7. 2.500 grams of metal X (molar mass 65.39 g/mole) was reacted with 100.0 mL of a 1.500 M HCI solution in a coffee cup calorimeter. The temperature went from 12.50 °C to 40.50 °C. Determine the reaction enthalpy per mole of metal X. The specific heat of the solution is 4.184 J/g o°C. Assume a solution density of 1.00 g/mL and a perfect system. 8. 20.12 grams of butane, C4H10, was combusted with oxygen in a bomb calorimeter. The temperature of 0.500 kilograms of water went from 5.00 oC to 25.89 °C. The specific heat of the water is 4.184 J/g °C. Assume a solution density of 1.00 g/mL. Determine the heat (kJ) evolved per mole of butane. Assume a perfect bomb calorimeter. See pre-laboratory letter e.

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
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Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...
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5. Why, on exothermic time-temperature graph, does the temperature eventually fall? 6. How many kJ of energy are required to change 1.00 m3 of pure water by 1.0 °C Assume a perfect system. The specific heat of the water is 4.184 J/g °C. The density of water is 1.000 g/mL. 1.00 m3 = 1000 Litres 7. 2.500 grams of metal X (molar mass 65.39 g/mole) was reacted with 100.0 mL of a 1.500 M HCI solution in a coffee cup calorimeter. The temperature went from 12.50 °C to 40.50 °C. Determine the reaction enthalpy per mole of metal X. The specific heat of the solution is 4.184 J/g o°C. Assume a solution density of 1.00 g/mL and a perfect system. 8. 20.12 grams of butane, C4H10, was combusted with oxygen in a bomb calorimeter. The temperature of 0.500 kilograms of water went from 5.00 oC to 25.89 °C. The specific heat of the water is 4.184 J/g °C. Assume a solution density of 1.00 g/mL. Determine the heat (kJ) evolved per mole of butane. Assume a perfect bomb calorimeter. See pre-laboratory letter e.
Transcribed Image Text:5. Why, on exothermic time-temperature graph, does the temperature eventually fall? 6. How many kJ of energy are required to change 1.00 m3 of pure water by 1.0 °C Assume a perfect system. The specific heat of the water is 4.184 J/g °C. The density of water is 1.000 g/mL. 1.00 m3 = 1000 Litres 7. 2.500 grams of metal X (molar mass 65.39 g/mole) was reacted with 100.0 mL of a 1.500 M HCI solution in a coffee cup calorimeter. The temperature went from 12.50 °C to 40.50 °C. Determine the reaction enthalpy per mole of metal X. The specific heat of the solution is 4.184 J/g o°C. Assume a solution density of 1.00 g/mL and a perfect system. 8. 20.12 grams of butane, C4H10, was combusted with oxygen in a bomb calorimeter. The temperature of 0.500 kilograms of water went from 5.00 oC to 25.89 °C. The specific heat of the water is 4.184 J/g °C. Assume a solution density of 1.00 g/mL. Determine the heat (kJ) evolved per mole of butane. Assume a perfect bomb calorimeter. See pre-laboratory letter e.
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