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 ã 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 î´hrxn in scientific notation. î´hrxn

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 () in a chemical reaction.

energy is released.

energy is absorbed.

The Thermochemical equation for the given reaction will be :

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 .

adding or remove a gaseous reactant or product changes the concentrations. if the concentration of reactant or product is increased, the system will shift away from the side in which concentration was increased (i.e. if the concentration of reactants is increased, the system will shift toward the products. if more products are added, the system will shift to form more reactants). conversely, if the concentration of reactant or product is decreased, the system will shift toward the side in which concentration was decreased (i.e. if reactants are removed, the system will shift to form more reactants. if the concentration of products is decreased, the equilibrium will shift toward the products).

explanation: