Glycine C2H5O2N is important for biological energy. The combustion of glycine is given by the equation, (show work please). 4C2H502N(s) + 9O2(g) → 8CO2(g) + 10H2O(l) +2N2(g)
ΔH° rxn = -3857 kJ
Given that ΔH° f[CO2(g)]=-393.5 kJ/mol, and ΔH° f[H2O(l)] = -285.8 kJ/mol. Calculate the enthalpy of formation ΔH f per mole of glycine.
Please help finals are coming soon and I need step by step directions to get this problem!!! I tried and I just can't get it :-(?
2014-07-19 12:23 am
回答 (1)
2014-07-19 12:52 am
✔ 最佳答案
ΔH° f of any element N2 and O2 is 0 kJ[8(393.5) + 10(285.8) + -3857 ] / 4 = 537.25 kj/mole
收錄日期: 2021-04-21 00:13:35
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