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.
a) The balanced thermochemical equation for the oxidation of sucrose can be written as follows:
C12H22O11(s) + 12O2(g) -> 12CO2(g) + 11H2O(g)
b) To calculate Delta Hrxn, we need to sum up the enthalpy changes of each individual bond broken and formed during the reaction. Given that the reaction releases 5.16 x 10^3 kJ/mol of sucrose, the Delta Hrxn would be -5.16 x 10^3 kJ/mol. The negative sign indicates that the reaction is exothermic.
c) To determine the amount of heat released per gram of sucrose oxidized, we need to convert the amount of heat released per mole (Delta Hrxn) to kJ/g.
First, we need to calculate the molar mass of sucrose (C12H22O11):
12 mol of carbon (12 g/mol) + 22 mol of hydrogen (1 g/mol) + 11 mol of oxygen (16 g/mol) = 342 g/mol
Now, we can calculate the heat released per gram of sucrose:
Delta Hrxn (kJ/mol) / molar mass of sucrose (g/mol) = -5.16 x 10^3 kJ/mol / 342 g/mol = -15.1 kJ/g
Therefore, the correct answer for part c) is -15.1 kJ/g. Note that the negative sign indicates the release of heat during the oxidation process.
a) The balanced thermochemical equation for the oxidation of sucrose in the body is:
C12H22O11(s) + 12O2(g) -> 12CO2(g) + 11H2O(g)
b) The value for Delta Hrxn is stated to be 5.16x10^3 kJ/mol. Since the equation is balanced for 1 mol of sucrose reacting, the value of Delta Hrxn remains the same, which is 5.16x10^3 kJ/mol.
c) To calculate the heat released per gram of sucrose oxidized, we need to use the molar mass of sucrose. The molar mass of sucrose (C12H22O11) can be calculated as follows:
12(12.01 g/mol) + 22(1.008 g/mol) + 11(16.00 g/mol) = 342.34 g/mol
Now, we can calculate the heat released per gram of sucrose:
Delta Hrxn = 5.16x10^3 kJ/mol
Heat released per gram = (Delta Hrxn / molar mass of sucrose) = (5.16x10^3 kJ/mol) / (342.34 g/mol) = 15.1 kJ/g
So, the answer for part c) is indeed 15.1 kJ/g.