HESS'S LAW AND ENTHALPY CHANGE CALCULATIONS
This page explains Hess's Law, and uses it to do some simple enthalpy
change calculations involving enthalpy changes of reaction, formation
and combustion. Hess's Law Stating Hess's Law Hess's Law is the most important law in this part of chemistry. Most calculations follow from it. It says . . .
Hess's Law is saying that if you convert reactants A into products B, the overall enthalpy change will be exactly the same whether you do it in one step or two steps or however many steps. If you look at the change on an enthalpy diagram, that is actually fairly obvious. In either case, the overall enthalpy change must be the same, because it is governed by the relative positions of the reactants and products on the enthalpy diagram. If you go via the intermediates, you do have to put in some extra heat energy to start with, but you get it back again in the second stage of the reaction sequence. However many stages the reaction is done in, ultimately the overall enthalpy change will be the same, because the positions of the reactants and products on an enthalpy diagram will always be the same. | |||||||||
Note: It is possibly confusing that I am switching between the terms enthalpy and energy. Enthalpy change is simply a particular measure of energy change. You will remember that the enthalpy change is the heat evolved or absorbed during a reaction happening at constant pressure. I have labelled the vertical scale on this particular diagram as enthalpy rather than energy, because we are specifically thinking about enthalpy changes. I could have just kept to the more general term "energy", but I prefer to be accurate. | |||||||||
You can do calculations by setting them out as enthalpy diagrams as
above, but there is a much simpler way of doing it which needs virtually
no thought. You could set out the above diagram as: The big advantage of doing it this way is that you don't have to worry about the relative positions of everything on an enthalpy diagram. It is completely irrelevant whether a particular enthalpy change is positive or negative. Warnings! Although most calculations you will come across will fit into a triangular diagram like the above, you may also come across other slightly more complex cases needing more steps. That doesn't make it any harder! You need to take care in choosing your two routes. The pattern will not always look like the one above. You will see that in the examples below. Enthalpy change calculations using Hess's Law cycles I can only give a brief introduction here, because this is covered in careful, step-by-step detail in my chemistry calculations book. Working out an enthalpy change of formation from enthalpy changes of combustion If you have read an earlier page in this section, you may remember that I mentioned that the standard enthalpy change of formation of benzene was impossible to measure directly. That is because carbon and hydrogen won't react to make benzene. | |||||||||
Important: If you don't know (without thinking about it too much) exactly what is meant by standard enthalpy change of formation or combustion, you must get this sorted out now. Re-read the page about enthalpy change definitions before you go any further - and learn them! | |||||||||
Standard enthalpy changes of combustion, ΔH°c are relatively easy to measure. For benzene, carbon and hydrogen, these are:
Why have I drawn a box around the carbon dioxide and water at the bottom of the cycle? I tend to do this if I can't get all the arrows to point to exactly the right things. In this case, there is no obvious way of getting the arrow from the benzene to point at both the carbon dioxide and the water. Drawing the box isn't essential - I just find that it helps me to see what is going on more easily. Notice that you may have to multiply the figures you are using. For example, standard enthalpy changes of combustion start with 1 mole of the substance you are burning. In this case, the equations need you to burn 6 moles of carbon, and 3 moles of hydrogen molecules. Forgetting to do this is probably the most common mistake you are likely to make. How were the two routes chosen? Remember that you have to go with the flow of the arrows. Choose your starting point as the corner that only has arrows leaving from it. Choose your end point as the corner which only has arrows arriving. Now do the calculation: Hess's Law says that the enthalpy changes on the two routes are the same. That means that: ΔH - 3267 = 6(-394) + 3(-286) Rearranging and solving: ΔH = 3267 + 6(-394) + 3(-286) ΔH = +45 kJ mol-1 | |||||||||
Note: If you have a good memory, you might remember that I gave a figure of +49 kJ mol-1 for the standard enthalpy change of formation of benzene on an earlier page in this section. So why is this answer different? The main problem here is that I have taken values of the enthalpies of combustion of hydrogen and carbon to 3 significant figures (commonly done in calculations at this level). That introduces small errors if you are just taking each figure once. However, here you are multiplying the error in the carbon value by 6, and the error in the hydrogen value by 3. If you are interested, you could rework the calculation using a value of -393.5 for the carbon and -285.8 for the hydrogen. That gives an answer of +48.6. So why didn't I use more accurate values in the first place? Because I wanted to illustrate this problem! Answers you get to questions like this are often a bit out. The reason usually lies either in rounding errors (as in this case), or the fact that the data may have come from a different source or sources. Trying to get consistent data can be a bit of a nightmare. | |||||||||
Working out an enthalpy change of reaction from enthalpy changes of formation This is the commonest use of simple Hess's Law cycles that you are likely to come across. In this case, we are going to calculate the enthalpy change for the reaction between ethene and hydrogen chloride gases to make chloroethane gas from the standard enthalpy of formation values in the table. If you have never come across this reaction before, it makes no difference.
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Note: I'm not too happy about the value for chloroethane! The data sources I normally use give a wide range of values. The one I have chosen is an average value from the NIST Chemistry WebBook. This uncertainty doesn't affect how you do the calculation in any way, but the answer may not be exactly right - don't quote it as if it was right. | |||||||||
In the cycle below, this reaction has been written horizontally, and
the enthalpy of formation values added to complete the cycle. |
Tuesday, 24 September 2013
HESS'S LAW AND ENTHALPY CHANGE CALCULATIONS
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