what is the enthalpy change in kilojoules for the combustion of 1 mol of ethanol, C2H5OH (l), to form gaseous carbon dioxide and gaseous water? use bond energies to calculate your answer. (hint: there is a double bond in carbon dioxide and oxygen)

the answer is supposed to be -1100 but i have no idea how to get it.

Look in your text for a table listing bond energies.
C2H5OH + 3O2 ==> 2CO2 + 3H2O

delta H = (sum B.E. reactants)-(sum B.E. products).

Reactants:
break 5 C-H bonds
break 1 C-C bond
break 1 C-O bond
break 1 O-H bond
break 1 O-O bond (and I used O=O)although it isn't exactly a double bond and that x 3 for 3 mols.

Products:
break 2 C=O bonds x 2 mols
break 2 O-H bonds x 3 mols

Using the table in my text at home I came up with -1022 kJ/mol C2H5OH but I have looked on the internet for numbers, too, and these numbers go all over the map. Use the above procedure but the numbers in your text or your notes and you should get close to -1100 kJ. Check my thinking. Check my work. I suggest you draw out the structures of C2H4OH, O2, CO2, and H2O and count the bonds.

That should be C2H5OH in the last line.

Using the bond energies from your text or notes, the enthalpy change for the combustion of 1 mol of ethanol, C2H5OH (l), to form gaseous carbon dioxide and gaseous water is -1100 kJ.

To calculate the enthalpy change, ΔH, for the combustion of 1 mole of ethanol, C2H5OH (l), to form gaseous carbon dioxide, CO2, and gaseous water, H2O, we can use bond energies.

1. Write out the balanced chemical equation for the combustion reaction:
C2H5OH + 3O2 → 2CO2 + 3H2O

2. Identify the bonds present in the reactants and products and calculate the bond energies. Consult a table or your textbook for the bond energies. Here are the bond energies needed for this calculation:

Reactants:
- 5 C-H bonds in C2H5OH
- 1 C-C bond in C2H5OH
- 1 C-O bond in C2H5OH
- 1 O-H bond in C2H5OH
- 1 O-O bond in O2 (considered as O=O, double bond)

Products:
- 2 C=O bonds in CO2
- 2 O-H bonds in H2O

3. Calculate the sum of the bond energies for the reactants and products:
Reactants: (5 × C-H bond energy) + (1 × C-C bond energy) + (1 × C-O bond energy) + (1 × O-H bond energy) + (1 × O-O bond energy) × 3
Products: (2 × C=O bond energy) × 2 + (2 × O-H bond energy) × 3

4. Subtract the sum of the bond energies of the products from the sum of the bond energies of the reactants:
ΔH = (Sum of bond energies of reactants) - (Sum of bond energies of products)

By using the bond energies given in your textbook or notes, you should be able to calculate the ΔH value.

To calculate the enthalpy change for the combustion of 1 mol of ethanol (C2H5OH), you need to use bond energies of the different bonds involved in the reaction.

First, let's write out the balanced equation for the combustion reaction:
C2H5OH + 3O2 → 2CO2 + 3H2O

The enthalpy change (ΔH) is given by the formula:
ΔH = (sum of bond energies of reactants) - (sum of bond energies of products)

Now, let's calculate the bond energies for the reactants:
- Break 5 C-H bonds in ethanol (C2H5OH)
- Break 1 C-C bond in ethanol (C2H5OH)
- Break 1 C-O bond in ethanol (C2H5OH)
- Break 1 O-H bond in ethanol (C2H5OH)
- Break 1 O-O bond in oxygen (O2) and multiply it by 3 (since there are 3 O2 molecules in the reaction)

Next, calculate the bond energies for the products:
- Break 2 C=O double bonds in carbon dioxide (CO2) and multiply it by 2 (since there are 2 CO2 molecules in the reaction)
- Break 2 O-H bonds in water (H2O) and multiply it by 3 (since there are 3 H2O molecules in the reaction)

Using the relevant bond energies from your text or notes, calculate the sum of the bond energies for the reactants and products, and then subtract the sum of the bond energies of the products from the sum of the bond energies of the reactants.

By following this procedure, using the given hint and the bonds mentioned, you should arrive at an enthalpy change of approximately -1100 kJ/mol for the combustion of 1 mol of ethanol. It's always good to check your thinking and work, and you can draw out the structures of the molecules involved to count the bonds accurately.