[megh44]

for the question....use the thermochemical equation for the combustion of glycine and other deltaH*f values to determine the deltaH*f of glycine...

i'm not sure what i am suposed to do...
i created the thermochemical equation but i am not sure what they mean by the deltaH*f of glycene does it mean hess's law...because then i am not sure how to make my other equations?

as well in another question it says this:
the the deltaH*combustion of sucrose (c12H22O11) is -5640.9 kj/mol. write the thermochemical equation for the combustion of sucrose. Calculate the standard heat of formation of this compound.

again i have the thermo chemical equation but what do they mean, what are they looking for when they say the standard heat of formation of this compound?

[enahs]

 n Glycine +  n O₂ -> n X? + n Y?      Δ-#

Reverse the reaction

n X + n Y -> n Glycine + n O₂    -(Δ-#)

You know have the ΔH for the products Glycine and oxygen.
You also know that the total ΔH is the sum of the products minus the sum of the reactants, right? Why do you know this? You can then get X, Y and O2 from your standard enthalpy of formations from the back of your book, solve for Glycine (and remember to balance it first and account for the n's when doing the calculations, as the standard enthalpy of formation is for 1 mol)

The other question can be worked in the same manner.