Sucrose (C12H22O11, table sugar) is oxidized in the body by O2 via a complex set of reactions that ultimately produces CO2 (g) and H2O (g) and releases 5.16x10^3 kJ/mol sucrose.
a) Write a balanced thermochemical equation for this reaction. Make sure to include the physical state of each reactant and product........>>>>>>..........
b)Enter the answer for Delta Hrxn ........................answer in SCIENTIFIFIC NOTATION in kJ Moles
c) How much heat is released per gram of sucrose oxidized? ...................... answer in kJ/g
is b.....-5.16 x 10^3
is .c..............15.1 kJ/g ??? thank you.
responded below.
a) To write a balanced thermochemical equation for the oxidation of sucrose, we first need to determine the reactants and products. From the given information, the reactants are C12H22O11 and O2, and the products are CO2 and H2O.
The balanced equation for the reaction can be written as:
C12H22O11(s) + 12 O2(g) -> 12 CO2(g) + 11 H2O(g)
b) Delta Hrxn represents the change in enthalpy (heat) during the reaction. Given that the reaction releases 5.16x10^3 kJ/mol of sucrose, the value of Delta Hrxn is -5.16x10^3 kJ/mol. The negative sign indicates that the reaction is exothermic, meaning it releases heat.
c) To find the amount of heat released per gram of sucrose oxidized, we need to calculate the molar mass of sucrose and then convert it to grams.
The molar mass of sucrose (C12H22O11) can be calculated by multiplying the atomic masses of each element and summing them up:
Molar mass of C12H22O11 = (12 * 12.01) + (22 * 1.01) + (11 * 16.00) = 342.3 g/mol
Now, we can calculate the amount of heat released per gram of sucrose:
Heat released per mole of sucrose = -5.16x10^3 kJ/mol
Heat released per gram of sucrose = (Heat released per mole of sucrose) / (Molar mass of sucrose)
Heat released per gram of sucrose = (-5.16x10^3 kJ/mol) / (342.3 g/mol) ≈ -15.1 kJ/g
Therefore, the answer for part c is approximately -15.1 kJ/g. It is negative because the reaction releases heat.