The amino acid glycine, C2H5NO2, is one of the compounds used by the body to make proteins. The

Question

equation for its combustion is
4C2H5NO2(s) + 9O2(g) -------------> 8CO2(g) + 10H2O(l) + 2N2(g)
For each mole of glycine that burns, 973.49 kJ of heat is liberated. Use this information plus values of Hof for the products of combustion to calculate Hof
for glycine.

Answer 1

dHrxn = 973.49 kJ/mol x 4 = ?
dHrxn = (n*dHof products) - (n*dHof reactants)
You know dHrxn dHo of all but glycine. Substitute and solve for dHof glycine.