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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

queen_honey_blossom answered 1 year ago
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