8.000g of Compound X with molecular formula C4H10 are burned in a constant-pressure calorimeter containing 30.00kg of water at 25°C . The temperature of the water is observed to rise by 2.905°C . (You may assume all the heat released by the reaction is absorbed by the water, and none by the calorimeter itself.) Calculate the standard heat of formation of Compound X at
8.000g of Compound X with molecular formula C4H10 are burned in a constant-pressure calorimeter containing 30.00kg of water at 25°C . The temperature of the water is observed to rise by 2.905°C . (You may assume all the heat released by the reaction is absorbed by the water, and none by the calorimeter itself.) Calculate the standard heat of formation of Compound X at
Chemistry: Principles and Practice
3rd Edition
ISBN:9780534420123
Author:Daniel L. Reger, Scott R. Goode, David W. Ball, Edward Mercer
Publisher:Daniel L. Reger, Scott R. Goode, David W. Ball, Edward Mercer
Chapter5: Thermochemistry
Section: Chapter Questions
Problem 5.63QE: A 0.470-g sample of magnesium reacts with 200 g dilute HCl in a coffee-cup calorimeter to form...
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8.000g of Compound
X
with molecular formula
C4H10
are burned in a constant-pressure calorimeter containing
30.00kg
of water at
25°C
. The temperature of the water is observed to rise by
2.905°C
. (You may assume all the heat released by the reaction is absorbed by the water, and none by the calorimeter itself.) Calculate the standard heat of formation of Compound
X
at
25°C
.
Be sure your answer has a unit symbol, if necessary, and round it to the correct number of significant digits.
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