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.
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 6.109QP: A 21.3-mL sample of 0.977 M NaOH is mixed with 29.5 mL of 0.918 M HCl in a coffee-cup calorimeter...
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Question 7
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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