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Question

The heat of formation of C2H5OH(l) is -66 kcal/mole. The heat of combustion of CH3OCH3(g) is -348 kcal mole, ΔHf for H2O and CO2 are - 68 kcal/mole and -94 kcal/mole respectively. Then determine the ΔH for the isomerisation reaction C2H5OCH3(g), and ΔE for the same are at T = 25C

A
ΔH=22kcal/mole,ΔE=21.408kal/mole
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B
ΔH=33kcal/mole,ΔE=21.408kal/mole
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C
ΔH=44kcal/mole,ΔE=21.408kal/mole
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D
ΔH=22kcal/mole,ΔE=56.408kal/mole
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Solution

The correct option is A ΔH=22kcal/mole,ΔE=21.408kal/mole
2CO2+3H2OC2H5OH+O2 ΔH1=+66kcal--------1
CH3OCH3(g)+O22CO2+3H2O ΔH2=348Kcal -----2
ΔH(H2O)=68kcal
ΔH(O2)=94kcal
ΔHofreaction2=348(3(68)+2(94))=44kcal
By addition of of reactions
CH3OCH3+O2+2CO2+3H2OC2H5OH+O2+2CO2+3H2O
ΔH=+6644=22kcal
ΔE=21.408kcal/mol

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