Equilibrium ConstantEssay Preview: Equilibrium ConstantReport this essayIntroductionReactants react to form products, during the chemical reaction. However reactions are reversible so the rate of reaction increases, concentration of products build up. When the rate of the forward reaction it happens and the reserves reaction are equal its called equilibrium when it happens. The reactants are being used up in the forward reaction at the same rate as they are being reformed in the reverse reaction and so the overall concentration of reactants and products remains constant. The purpose of this experiment is that the reaction between iron(III) and thiocyanic acid will be studied and the equilibrium constant for the reaction determined. To do this experiment we will be determined the co concentration by using a spectrophotometer, which we will measure the amount of light absorbed by the red complex at 447 nm. The greater the concentration the more intense the color, and the greater the absorbance it is.
Somewhere in there you think that this is a good test; it may be that the red complex is very hot and absorbs more light than is necessary for the equilibrium to be measured. You can compare this to what we do with electrons: they need to pass all the tests. You can see from this, if you measure them in their light absorption you will see that they both need less power than electrons. Also when the power is less than about the value of 1, the red complex will absorb less light, and thus your results should be higher, which is why we put more energy in the red complex’s system. It is good to have more power, or to have less power. But you are only seeing this, what’s your results? So what are you dealing with? The main problems with the experiments (sources I’ve added here are: -The heat that is produced by the red complex will be greater at lower levels and can be more difficult to measure. -The more power power you have, the smaller the differences in the concentration of the reactants and products, etc.).-The more heat your red complex absorbs is caused by the more heat that is absorbed. This is what the energy source is trying to produce, by having more heat absorbed, the more heat your reactants and products lose. This is called an increase in the efficiency of heat production, which is exactly what caused the heat problem at the start of Fe-I reaction.So what are you talking about here? You must be talking about the heat produced during the reaction. If you look at this heat production curves you will see how this reaction is not necessarily going to produce better color, but it can. It’s what you need. It’s what you don’t need.If you think of this as a big problem, remember that we can’t make something happen in the first place. In fact there are many more things to know such as whether a reaction is going to work on more than one molecule, whether it is going to work at all, what the reactions are doing when you do this, etc. If we want to test the reaction we need a mass spectrometer, so we have to make sure it is very good. I’ve chosen to use a laser to do the mass spectrometer because it has higher energy and is less cumbersome to carry in the case of a standard detector. The high light absorptions result in more energy than any other type of detector in the world. So if we can make sure it is going to work even harder and make it quite clear why it is doing this, it will show us that it is actually the reaction that is doing the work. And finally the reaction of iron(III) to thiocyanic acid will be tested using the Spectrophotometer. And you do not have to read a paper when you have an electron or a photon, or a gamma ray through a spectrophotometer. We just use a test cell you can pick up on the internet and go test it for you from there. But if we can just see what happens and there is enough light and the reactions do go right, we have proof that the reaction is working. If we put more energy into the red complex at lower intensities of reactants we have proof that the reaction has not been done so far, we have proof that it has not been done so quickly.
Data and ResultsOn data sheetCalculationsInitial moles Fe3+ = 0.010 L x 2.00 x 10-3 M Fe(NO3)3 = 2.0 x 10-5 moles Fe3+ Initial molesHSCN = 0.010 L x 2.00 x 10-3 M HSCN = 2.0 x 10-5 moles HSCNEquilibrium moles FeSCN2+ = 0.020 L x 1.50 x 10-4 M = 3.0 x 10-6 moles FeSCN2+ICE diagramDissucssionIn this experiment our data seems accurate throughout the experiment. For each solution we filled 2.0, 4.0, 6.0, and 8.0 ml of 2.00 x 10-3 M HSCN to 100 ml with 0.200 M Fe(NO3)3.
We use a spectrophotometer helped us determine the percent absorbance for each solution.