Anonymous
Anonymous asked in Science & MathematicsChemistry · 1 decade ago

How do I calculate the enthalpy of formation of ethanol?

I am very confused on how to calculate this. Please show me the process with explanations. Thanks!

Calculate the standard enthalp of formation of ethanol C2H5OH (l) from the heat of combustion of ethanol, which is -1368 kJ/mol, by using tabulated standard enthalpies of formation for CO2 (g) and H20 (l).

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  • 1 decade ago
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    The combustion of C2H5OH is as follows:

    C2H5OH (l) + 3O2 (g) -----> 2CO2 (g) + 3H2O (l)

    The heat of combustion of ethanol is -1368 kJ/mol.

    Heat of formation of CO2 (g) = -393.509 kJ/mol

    Heat of formation of H2O (l) = -285.83 kJ/mol

    Total enthalpy change = total heat of formation of CO2 reaction + total heat of formation of H2O in reaction

    Therefore, total enthalpy change = 2(-393.509) + 3(-285.83) = -787.018 + (-857.49)

    = -1644.508 kJ/mol

    Obviously, there is a difference between the total enthalpy change of the reaction and the heat of combustion of ethanol. This difference is the enthalpy of formation of the ethanol.

    The difference = -1644.508 - (-1368) kJ/mol = -276.51 kJ/mol

    Therefore, enthalpy change of formation of ethanol = -276.51 kJ/mol

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  • 3 years ago

    Enthalpy Of Combustion Of Ethanol

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  • 3 years ago

    Enthalpies Of Formation Table

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  • Anonymous
    5 years ago

    RE:

    How do I calculate the enthalpy of formation of ethanol?

    I am very confused on how to calculate this. Please show me the process with explanations. Thanks!

    Calculate the standard enthalp of formation of ethanol C2H5OH (l) from the heat of combustion of ethanol, which is -1368 kJ/mol, by using tabulated standard enthalpies of formation for CO2 (g) and...

    Source(s): calculate enthalpy formation ethanol: https://trimurl.im/j36/how-do-i-calculate-the-enth...
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  • HPV
    Lv 7
    1 decade ago

    The balanced equation for the combustion of ethanol (l) is

    C2H5OH(l) + 3O2(g) ==> 2CO2(g) + 3H2O(l) . . .delta H = -1368 kJ

    The delta H for any reaction can be calculated as

    delta H reaction = sum of delta H of formation of products - sum of delta H of formation of reactants

    From tables:

    delta H f CO2(g) = -393.5 kJ/mole

    delta H f H2O(l) = -285.8 kJ

    delta H f O2(g) = 0

    delta H reaction = ((2 moles CO2)(-393.5 kJ/mole) + (3 moles H2O)(-285.8 kJ/mole)) - ((1 mole C2H5OH)(delta H f C2H5OH(l))

    -1368 kJ = (-787.0 kJ - 857.4 kJ) - (delta H f C2H5OH(l)

    -276.4 kJ = delta H f C2H5OH(l)

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  • 4 years ago

    answer is -1235

    • Alexa2 years agoReport

      can you explain this?

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