Question
In: Chemistry
Glycine, C2H5O2N, is important for biological energy. The combustion reaction of glycine is described by the...
Glycine, C2H5O2N, is important for biological energy. The combustion reaction of glycine is described by the following thermochemical equation. 4C2H5O2N(s) + 9O2(g) → 8CO2(g) + 10H2O(l) + 2N2(g) ΔH°rxn=-3857 kj/mol. What is the energy transfer in the oxidation of 17.00g of glycine?
Solutions
Expert Solution
4 C2H5O2N(s) + 9O2(g) ------------------- 8 CO2(g) + 10 H2O(l) + 2 N2(g) ΔH°rxn=-3857 kj/mol
4 mole
molar mass of glycine= 75.07 g/mole
mass of one mole of glycine = 75.07 grams
mass of 4 moles of glycine = 4 x75.07 = 300.28 grams
according to equation
energy is transferred from 300.28 grams of glycine = 3857 Kj
enegy is transfereed from 17.00 grams of glycine = ?
= 3857 x 17.00/300.28 = 218.36 KJ
Energy transferred during the oxidatioong glycine 218.36 KJ
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