Answer to Question #168383 in General Chemistry for Dawson

Question #168383

Sucrose (C12H22O11, table sugar) is oxidized in the body by O2 via a complex set of reactions that ultimately produces CO2(g) and H2O(l) and releases 5.16 × 103 kJ of heat per mole of sucrose...

(a) Write a balanced thermochemical equation for this reaction. Include the physical state of each reactant and product.


Enter your answer for ΔHrxn in scientific notation.


(b) Calculate the energy change per gram of sucrose for this combustion reaction. Do not answer in scientific notation.

1
Expert's answer
2021-03-05T03:27:50-0500

Thermochemical equation : it is a chemical reaction equation in which states of all reactants and products are written along with the energy change or enthalpy change "\\Delta H" in a chemical reaction.

"\\Delta H" = negative energy is released

"\\Delta H" = positive energy is absorbed

The Thermochemical equation for the given reaction will be :

C12H22O11(aq) + 12O2 (g) "\\to" 12CO2 (g) + 11H2O(l)

One mole of sucrose is oxidized by the 12 moles of oxygen to give 12 moles of carbon-dioxide, 11 moles of water and heat energy. the value of theis energy is equal the  that is "\\Delta H_{rxn}" that is -5.16×103 KJ


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