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Calculate DeltaH for the following homogeneous gaseous reaction CH_(3)COCH_(3)+2O_(2) to CH_(3)COOH+CO_(2)+H_(2)O from the following data: Bond energies : C-H=99 "kcal" C-C=83 "kcal" C=O=173 "kcal" O=O=118 "kcal" C-O=84 "kcal" O-H=110 "kcal" |
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Answer» Solution :We have `H-overset(H)overset(|)UNDERSET(H)underset(|)(C )-overset(O)overset(||)(C )-overset(H)overset(|)underset(H)underset(|)(C )-H+2O=O to H-overset(H)overset(|)underset(H)underset(|)(C )-overset(O)overset(||)(C )-O-H+O=C=O` `+H-O-H`, `DeltaH=?` For REACTANTS Bond energy of 6 moles of C-H bonds `=6xx99` kcal Bond energy of 2 moles of C-C bonds `=2xx83` kcal Bond energy of 1 mole of `C=O` bonds `=1xx173` kcal Bond energy of 2 moles of O=O bonds `=2xx118` kcal For products Energy of formation of 3 moles of C-H bonds `=-3xx99` kcal Energy of formation of 1 mole of C-C bonds `=-83` kcal Energy of formation of 1 mole of C=O bonds `=-173` kcal Energy of formation of 1 mole of C-O bonds `=-84` kcal Energy of formation of 1 mole of O-H bonds `=-110` kcal Energy of formation of 2 moles of C=O bonds `=-2xx173` kcal Energy of formation of 2 moles of O-H bonds `=-2xx110` kcal Adding up, we get `DeltaH` of the required equation i.e., `DeltaH=-144` kcal |
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