EXP #34.docx - Unk 1 Ridge Unk CHEM 112 M/W 7:35 Farnum...

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Unk 1Ridge UnkCHEM 112M/W 7:35 FarnumMarch 22, 2019Experiment #34 An Equilibrium ConstantConclusion: Our equilibrium constant for the reaction was KC=256.012 with an RSD% = 19.16% and a percent error of 80.29%. I am not very confident in the quality if my results, because there were many factors that affected the outcome of the results, but I am confident in the quality of precision made in this lab.
Unk 2Abstract:In today’s experiment we use a technique that is called spectrophotometric analysis, this technique involves the use of electromagnetic radiation waves that hit in object at different wavelengths in which some is absorbed and some is transmitted. The objective of this experiment is to determine the equilibrium constant of a chemical system using a the amount of light that is been given off by the spectrophotometer in order to determine the concentration of the solution, its also known as transmittance. The data collected would then be graphed and analyzed in order to determine the equilibrium constant for the solution. Electrons in molecules are structured in a way that it would allow the transmission of some of light radiation through it. Each molecular formation allows for a certain amount of light transmittance depending on its concentration, they are propionate to each other. In order to determine The intensities of the transmitted light we use a Spectrophotometer, which is capable to capturing light intensities that range from 400 to 700 nm. We know from looking at the experiment that there are three factors that can affect the amount of light transmitted through. One, The concentration of the absorbing substance. Two, the sickness of sample containing the absorbing substance. Three, the probability of light absorption five absorbing substance. The theoretical equilibrium constant thatI found online was 142. The experimental equilibrium constant was 256.022 with an RSD% of 19.171 and it had a % error of 80.2969 %. Introduction:
Unk 3In today's experiment we are using a spectrophotometer in order to determine concentrations of solutions through their absorbance. the Substances are colored when they absorb a particular wavelength of light in the visible light region and transmit the other wavelengths. One of the complex ions such as FeNCS2+which was used today, usually absorb light in the visible range; the color we see is the sum of the transmitted wavelengths. A spectrophotometer is an instrument that separates visible light into its component wavelengths and then measures the amount of light absorbed by the solution at a particular wavelength. The spectrophotometer is measuring the amount of light that is transmitted through your sample and hits the detector as a percentage of the light transmitted, this is only possible to get accurate reading when we use a blank solution in order to be our base point. Our Blank sample was a 0.2 M Fe(NO3)3, and then we diluted it down to 25 ml using 0.1M HNO3. The absorbance rate is

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