I don't think so.
dHrxn = (n*dHf products) - (n*dHf reactants)
4*-973.49 = (8*dHfCO2 + 10*dHf H2O) - (4*dHf glycine)
Solve for dHf glycine
The amino acid glycine, C2H5NO2, is one of the compounds used by the body to make proteins. The equation for its combustion is
4C2H4NO2(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 ΔHf° for the products of combustion, to calculate ΔHf° for glycine.
My answer:
973.49*4 = 3893.96kJ/mol
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