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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. δhrxn

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Answer :

When sucrose is oxidized by the oxygen gas to produces carbon dioxide and water as a product.

The balanced thermochemical equation for this reaction is,

[tex]C_{12}H_{22}O_{11}(s)+12O_2(g)\rightarrow 12CO_2(g)+11H_2O(l)[/tex]

  • Enthalpy of reaction : It is defined as the amount of energy or heat absorbed or released per mole in the reaction.

The [tex]\Delta H_{rxn}[/tex] is represented in scientific notation as,

[tex]\Delta H_{rxn}=5.16\times 10^3KJ/mole[/tex]

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