I don't know why it was marked wrong. This is what it said: Where is the 5.64 coming from? Is this a typo?(thank you)
HINT
To balance the equation, make sure that the number of each atom on the reactant side is the same as the number on the product side. Should the enthalpy change for this reaction have a positive sign or a negative sign? From the balanced thermochemical equations, how many moles of C12H22O11 (sucrose) are thermochemically equivalent to 5.64 x 10^3 kJ? Use this equivalent quantity as a conversion factor to calculate how much heat is released per gram of sucrose oxidized . Make sure all your units cancel out and the signs are correct in your calculations.
THIS WAS THE 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 (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.•chemistry - DrBob222, Sunday, October 18, 2015 at 1:32pm
C12H22O11(s) + 12O2(g) ==> 12CO2(g) + 11H2O(g) dH = -5.16E-3 kJ
b is -5.16E+3 kJ/mol
c is right
2 answers
4 answers