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...

Question

(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

a) C₁₂H₂₂O₁₁(aq) + 12O₂(g) ==> 12CO₂(g) + 11H₂O(l) + 5.16x10³ kJ ... balanced thermochemical equation

b) molar mass sucrose = 342 g/mol

5.16x10³ kJ/mol sucrose x 1 mol sucrose / 342 g = 1,764,720 kJ = 1,760.000 kJ (3 sig. figs.)