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 à 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. â enter your answer for δhrxn in scientific notation. δhrxn

Answer 1

Explanation:

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 :

$C_{12}H_{22}O_{11}(aq)+12O_2(g)\rightarrow 12CO_2(g)+11H_2O(l),\Delta H_{rxn}=-5.16\times 10^{3} kJ$

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 $\Delta H_{rxn}$ that is $-5.16\times 10^{3} kJ$.