Use bond energies to estimate the heat for the
combustion of 2.6 g of acetylene gas C2H2 to form carbon
dioxide and water vapor
First we convert 2.6 g of acetylene to mole.
molar mass of acetylene = 26.04 g/mol
mass = 2.6
moles = 2.6 / 26.04 g/mol =0.099 g/mol g/mol
The heat for the combustion of 2.6g (0.1 mol) of acetylene C2H2 to form carbon dioxide and water vapor
The bond dissociation energies:-
BE(C–H) = 456 kJ/mol
BE(C≡C) = 962 kJ/mol
BE(O=O) = 499 kJ/mol
BE(C=O) = 802 kJ/mol
BE(O–H) = 462 kJ/mol
0.1(C2H2) + (5/2)O2 → 2CO2 + H2O
0.1(H-C C-H)+ 5/20=0 ---> 20=C=O + H-0-H
0.1[962 + (2)(456)] + (5/2)499 = (2)(2)(802) + (2)(462) +
E
E = (187.4+1247.5 - 4134) kJ/mol
E = 2699.1 kJ/mol kJ/mol
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