Combustion of C12H22O11(s) (sucrose or "table sugar") produces CO2(g) and H2O(l). When 1.43 g of sucrose is combusted in a constant volume (bomb) calorimeter, 23.6 kJ of heat is liberated. Calculate ΔE for the combustion of 6.05g of sucrose.
Combustion of C12H22O11(s) (sucrose or "table sugar") produces CO2(g) and H2O(l). When 1.43 g of sucrose is combusted in a constant volume (bomb) calorimeter, 23.6 kJ of heat is liberated. Calculate ΔE for the combustion of 6.05g of sucrose.
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
Chapter18: Thermodynamics And Equilibrium
Section: Chapter Questions
Problem 18.97QP: When 1.000 g of gaseous butane, C4H10, is burned at 25C and 1.00 atm pressure, H2O(l) and CO2(g) are...
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Combustion of C12H22O11(s) (sucrose or "table sugar") produces CO2(g) and H2O(l).
When 1.43 g of sucrose is combusted in a constant volume (bomb) calorimeter, 23.6 kJ of heat is liberated.
Calculate ΔE for the combustion of 6.05g of sucrose.
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