Experiment Spectrophotometric Equilibrium Constant

 

determination of equilibrium constant lab report

Feb 21,  · At equilibrium, the reactants turn into product and the products decompose into reactants at the same rate. This ratio of the products to reactants at equilibrium is represented by the equilibrium constant, or K. K is found by taking the concentration and order of the products and dividing by the concentration and order of the reactants. Determination of the Equilibrium Constant for the Iron (III) thiocynate Reaction Prelab Assignment Before coming to lab: After reading "Lab Notebook Policy and Format for Lab Reports" handout, complete in, your lab notebook the following sections of the report for this lab exercise: Title, Introduction, Materials/Methods and Data Tables. An. Determination of the Equilibrium Constant Kyle Miller December 11, 1 Purpose The purpose of this experiment is to determine the equilibrium constant for the reaction Fe3+ + SCN− FeSCN2+ and to see if the constant is indeed the same under different conditions. 2 Procedure.


Determining an Equilibrium Constant Using Spectrophotometry — Adam Cap


The equilibrium state can be categorized by stating its equilibrium constant as large, greater than one, determination of equilibrium constant lab report, or small, less than onebut not negative or zero.

A large Kc. A small Kc means that at equilibrium, the concentrations of the reactants will generally be greater than the concentrations of the products, meaning it is reactants favored, determination of equilibrium constant lab report. The relevant chemical equation for this lab is:.

The initial. When the chemical reaction reached equilibrium, the. Concentrations determination of equilibrium constant lab report measured, the value of the equilibrium constant was easily calculated. Finally, the concentrations of each sample in the experiment were calculated; so, the equilibrium constant was calculated.

To find the value of Kc, it is necessary to determine the concentration of several solutions at equilibrium. Light acts like a wave and has properties. The different wavelengths of light can be seen in the different colors. The entire electromagnetic determination of equilibrium constant lab report as shown in the figure below:.

The greater the concentrations of determination of equilibrium constant lab report ions, the greater the absorbance of the solution was. There were several factors that. This explained why the absorbance was linearly proportional to the factors that affected it, the thickness, the concentration, and the absorptivity, of a given.

The concentrations of the entire samples become part constant 3. If absorbance is plotted versus concentration, the slope will give the molar absorptivity constant per Beer's Law. If a solute obeys Beer's law, then the equation equation 3when graphed "Absorbance versus Concentration," yielded a.

Procedure Preparation for the Samples for the Calibration Curve The spectrophotometer was turned prior to the preparing of the solutions so that it. Six 25 mL volumetric flasks were first rinsed and dried to ensure that there was no residue from previous experiments. The volumetric flasks were then labeled blank and so that the order would not be confused. Following Table 1, 0. A plastic graduated cylinder was used to measure this solution. It was not cleaned after every used of the same liquid.

The solution was poured carefully and slowly. Fe NO3 3 was added to each volumetric flask. Using the same plastic graduated cylinder that was now cleaned and dried, the next solution was added to the volumetric flasks. Again, the same plastic graduated cylinder was used after it was cleaned and dried for the last solution that was added.

Once more, while. When the volumetric flasks were stirred or flipped over to mix the solution, careful consideration was taken into account because the lids. Each solution was stirred to make sure that the equilibrium was established throughout the solution. After carefully mixing the solution, each solution was poured into a cuvet. Each cuvet was filled about.

All six of the cuvets were brought to the spectrophotometer so that their absorbance could be, determination of equilibrium constant lab report. The first solution in the cuvet to be tested was the blank solution.

A Kimwipe was used to wipe down the sides of the cuvet to remove any liquid or fingerprints. The cuvet was handled only on the sides that were grooved since the clear sides were used to test for. For maximum absorption of the wavelength the spectrophotometer was set at nm. No adjustments were made for the remainder of the experiment. Preparations for the Test Solutions. The test determination of equilibrium constant lab report were prepared according to Table 2 in six clean 10 mL volumetric flasks in the identical fashion as the ones.

Molar concentrations for this part of the experiment were different from the first part. A new blank solution was created and used to recalibrate the spectrophotometer for this. Determining the absorbance of the test samples, determination of equilibrium constant lab report were followed from the previous section.

The data gathered from the second part of the experiment was used for the calculations of Kc 1. NaSCN Mol. SCN- reacted 1 4, determination of equilibrium constant lab report. Average Kc Kc First step was to calculate the absorbance of the standard solutions for the test. The accepted value is The standard deviation for the results is This means that the data plotted will most likely lie in the range of. Looking at the Kc values, this statement is true for the values that were calculated in this experiment.

The relative standard deviation for this experiment was. From a practical standpoint, producing a given chemical product, it would be essential to know the Kc of a reaction so that the yield. The reaction essentially "goes to completion. If Kc was very. The reaction does not occur to any great extent. Most of the reactants remain. When Kc was not very large or not very small close to a value of 1then approximately equal amounts of reactants and products.

The significance of the experimental results showed that the Kc was large so that this reaction was products favored 6.

The cylinder was to measure the liquids was not washed and dried after each use of the same solution. Also, the lids had to be washed and dried after each used. The cuvets that were used had to be checked very carefully since quite a few of them were damaged with scratches and others defects.

With all of these. The standard deviation of the experiment was This stated that most of the data plotted would be within The standard deviation and the error analysis figures helped to reinforce that mistakes were made while conducting this experiment. The plotted concentration points that remained and were graphed creating points that were closer to the line.

The R2 value became. This was accomplished by using a. From which equilibrium concentrations were calculated with the Beers Law. Determination of an equilibrium constant. Read Free For 30 Days. Equilibrium Constant Report Example 4. Uploaded by jim gorman. Description: Equilibrium Constant Report Example 4. Flag for inappropriate content. Related titles. Carousel Previous Carousel Next.

Chem Spectrophotometric Determination of the Equilibrium Constant of a Reaction. Jump to Page. Search inside document. The experiment equilibrium constant was derived from the average of the trial results. This chemical reaction created a state of chemical equilibrium. A large Kc equilibrium constant means that at equilibrium, the concentrations of the products will generally be greater than the concentrations of the reactants, meaning it is products favored.

The stoichiometry determination of equilibrium constant lab report reactant: reactant: product ; the moles of each reactant was used up in the reaction equaled to the moles of product formed equation 1.

The initial concentrations of the known reactants were subtracted to find the moles of reactant remaining at equilibrium. When the chemical reaction reached equilibrium, the concentrations of reactants and products no longer change with time 2.

A spectrophotometric method of analysis involves using light waves. This method requires a calibration curve using samples of known concentration. This can be done by spectroscopy. This was accomplished by using a spectrophotometer, an instrument used to measure the amount of light that passes through a sample 1. The entire electromagnetic spectrum as shown in the figure below: Figure 2 Electromagnetic Spectrum The visible light region of the spectrum is small compared to the range of wavelengths.

The reactants in the solutions absorbed the light waves. There were several factors that affected the absorbance of light: concentration of the solution, thickness of the sample of solution, and the probability of the light absorbance of the solution 4. Once the absorbency of the solutions was determined Beers law was applied.

 

Equilibrium Lab Report by Erichelle Goitia on Prezi

 

determination of equilibrium constant lab report

 

Answer to Determination of an Equilibrium Constant Lab Help with calculations? How to determine [Fe(SCN)2+, slope from graph Determination of the Equilibrium Constant for the Iron (III) thiocynate Reaction Prelab Assignment Before coming to lab: After reading "Lab Notebook Policy and Format for Lab Reports" handout, complete in, your lab notebook the following sections of the report for this lab exercise: Title, Introduction, Materials/Methods and Data Tables. An. Determination of an Equilibrium Constant. Introduction. A state of chemical equilibrium exists when the rate of the forward reaction is equal to the rate of the reverse reaction. Once equilibrium has established itself, the amounts of products and reactants are constant. For this lab report, you will need to include a title, abstract.