When 1.535 g of methanol (CH3OH) was burned in a constant-volume bomb calorimeter, the water temperature rose from 20.27oC to 26.87oC. If the mass of water surrounding the calorimeter was exactly 1000 g and the heat capacity of the bomb calorimeter was 1.75 kJ/oC, calculate the molar heat of combustion of CH3OH. The specific heat of water is 4.184 J/g·oC. A. -8.17 x 105 kJ/mol B. -817 kJ/mol C. 1.88 kJ/mol D. 817 kJ/mol
When 1.535 g of methanol (CH3OH) was burned in a constant-volume bomb calorimeter, the water temperature rose from 20.27oC to 26.87oC. If the mass of water surrounding the calorimeter was exactly 1000 g and the heat capacity of the bomb calorimeter was 1.75 kJ/oC, calculate the molar heat of combustion of CH3OH. The specific heat of water is 4.184 J/g·oC. A. -8.17 x 105 kJ/mol B. -817 kJ/mol C. 1.88 kJ/mol D. 817 kJ/mol
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Chapter6: Thermochemisty
Section: Chapter Questions
Problem 6.75QP: A sample of ethanol, C2H5OH, weighing 2.84 g was burned in an excess of oxygen in a bomb...
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When 1.535 g of methanol (CH3OH) was burned in a constant-volume bomb
calorimeter, the water temperature rose from 20.27oC to 26.87oC. If the mass
of water surrounding the calorimeter was exactly 1000 g and the heat
capacity of the bomb calorimeter was 1.75 kJ/oC, calculate the molar heat of
combustion of CH3OH. The specific heat of water is 4.184 J/g·oC.
A. -8.17 x 105 kJ/mol
B. -817 kJ/mol
C. 1.88 kJ/mol
D. 817 kJ/mol
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