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Use the bond dissociation energies in Table 8.3 in the textbook to calculate an approximate heat of reaction, Delta H degree in kilojoules, for the industrial reaction of ethanol with acetic acid to yield ethyl acetate (used as nail-polish remover) and water.
Use the bond dissociation energies in Table 8.3 in the textbook to calculate an approximate heat of reaction, Delta H degree in kilojoules, for the industrial reaction of ethanol with acetic acid to yield ethyl acetate (used as nail-polish remover) and water.
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Patrina SchowalterLv2
7 Jul 2019
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Related questions
The value of Kc for the reaction of acetic acid with ethanol is 3.4 at 25âC:
CH3CO2H(soln)+ | C2H5OH(soln)â | CH3CO2C2H5(soln)+H2O(soln)Kc=3.4 |
Acetic acid | Ethanol | Ethyl acetate |
Part A
How many moles of ethyl acetate are present in an equilibrium mixture that contains 3.7 mol of acetic acid, 6.4 mol of ethanol, and 12.5 mol of water at 25 âC?
Part B
Calculate the number of moles of all reactants and products in an equilibrium mixture prepared by mixing 1.00 mol of acetic acid and 10.00 mol of ethanol.