Answer to Question #168383 in General Chemistry for Dawson

Question

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 ΔH_rxn in scientific notation.

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

Answer 1

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