In this experiment, rate laws and graphs help calculate the oxidation of food dyes by sodium hypochlorite. During the experiment the linear relationship between absorbance…
The materials were first acquired then with the groups in the class each team was given a test solution to create and acquire information from then all the information was put together in order to save time. Specifically the group created test solutions #8, #9, and #10. Once the solutions were created, they were stirred to ensure that the reaction had fully occurred. Then the solutions were placed in a spectrometer that was set to a wavelength of 450nm. The absorption for each of the solutions was measured and recorded. With the whole data collected from the overall group a calibration curve was created from the reference solutions and the concentrations of FeSCN2+ at equilibrium was demined by finding the absorbance from the test solutions on the calibration curve and tracing it to their concentrations. The initial concentrations of Fe3+ and SCN- were found using the M1V1 = M2V2 equation along with the concentration of FeSCN2+ used in the calibration curve. Then using the chart that organizes the initial, change, and equilibrium concentrations of a specific products and reactions; the concentration of Fe3+ and SCN- was determined. With the concentrations of the products and the reactants the Keq was determined.…
The objectives of this lab include- illustrating the use of the spectrophotometer in chemical analysis, and generating a standard, or calibration curve, then using that curve to determine the value of an unknown substance. The spectrophotometer is one of the most powerful tools used in chemistry to find the concentration of substances in solution. It compares the colors of a known and an unknown solution, that comparison then leads to a quantitative estimate of the concentration of trace amounts of colored materials in that solution.…
The purpose of this experiment is to understand the components of a reaction at chemical equilibrium and use Le Chatelier’s principle to predict the direction an equilibrium position will shift upon changes in the concentration, temperature, and pressure. It was determined that in the equilibrium of chromate and dichromate it is an exothermic reaction and in the equilibrium of ferrocyanide and ferric ferrocyanide that it is an equilibrium shift to the left after adding NaOH.…
Dry, sublimed ferrocene (93 mg) was added to a reaction tube. Later, 0.35 mL of acetic anhydride and 0.1 mL of 85% phosphoric acid were also added. The reaction tube was capped using a septum, and a syringe needle was poked through. This was warmed over a steam bath and stirred for 10 minutes after it began to boil, forming a dark brown color. The tube was then cooled to room temperature, then further cooled in ice. A solution of 0.5mL was added, dropwise w/ mixing. 3M NaOH was added until the pH of the solution was neutral. The product was vacuum filtrated and pressed dry.…
Abstract: This experiment helps determine the rate of reaction of crystal violet while it reacts with sodium hydroxide with respect to crystal violet. The amount of sodium hydroxide is varied in this experiment while crystal violet is kept at a constant. The transmittance of crystal violet is observed and recorded using a colorimeter and the data obtained is used to plot graphs which are manipulated using LoggerPro software to produce the desired outcome; rate of reaction of crystal violet. Upon completion of the experiment it was seen that the rate of reaction of crystal violet turned out to be 1 which meant the reaction was first order with respect to crystal violet. This was deduced upon plotting the graph of ln Absorbance versus time of crystal violet and by drawing the line of best fit, which showed that the slope graph was 1 which is the rate of reaction. This whole experiment was based upon the equation: Rate= k [CV+] [OH-], where k stands for the rate constant.…
Key quantities and properties for this experiment are summarized in Tables 1-3. Relevant chemical quantities and properties are presented in Table 1, table 2 contains the summary of characterization results. Table 3 contains the summary of the characterization results. Relevant experimental observations performed during the experiment are described in Table 4.…
This investigation used spectroscopy to evaluate light absorption in different solutions. A spectrophotometer was used in the lab to determine these values. A spectrophotometer is an apparatus used to “measure the absorption of radiation in the visible and UV regions of the spectrum and allows precise at a particular wave length” (Jones et al., 2007). The amount of light absorbed by a substance is directly in relation to the concentration of the solute and also the wavelength moving through the solute (Jones et al., 2007). This is commonly referred to as Beer’s Law and can be expressed as A= εl [C]. Beer’s Law equation measures the absorbency of light, making it an effective measure as spectrophotometers give exact values for absorbency (Jones et al., 2007).…
where [A]0 and [B]0 are the initial concentrations of C6H8O6 and [Fe(CN)6]3- and a=1 and b=2. From equation (5), it is possible to calculate the second-order rate constant k by plotting ln [A]/[B] against time (find slope of line where b=2 and a=1). EDTA in this experiment is used as a masking agent to hide metal ions that would normally interfere with the analysis in this reaction. Thus the absorbance of [Fe(CN)6]3- at time t is given by:…
It is necessary to determine the molar concentration of each of the three species in solution at equilibrium to fine the value of Keq, which depends only upon temperature. In order to have a successful evaluation of this equilibrium system, it is important to conduct three tests separately. This experiment is done into two sections. First, from the series of standard solution of FeSCN2+ was prepared varying concentration of SCN- and constant concentration of H+ and Fe+ that are in stoichiometric excess. The excess of H+ ions will ensure that Fe3+ has no engage in the reaction and excess of Fe3+ ions will make the SCN- ion which is a limiting reagent. In part ll the solution of unknown [SCN-] was analyze using the same procedure as in part…
After arranging all the solutions from palest to darkest in their respective treatments, the spectrometer would be needed. Starting with the palest and moving to the darkest, all absorbance was measured at 460 nm. Once all these readings are found, divide by 0.0078 to calculate the benzoquinone concentration (µm). Mean and standard deviation were both calculated using Microsoft Excel…
Spectroscopy is the study of matter interacting with electro-magnetic radiation (e.g. Light). In this lab, we will separate some light sources in to constituent colors and find out the wavelength of some atomic emissions. We will also try to compare the line spectra found from gas discharge tubes and flame emissions. Finally, we will measure the absorbance of Copper sulfate solution as a function of wavelength.…
For this paper you must have: ● the Periodic Table/Data Sheet, provided as an insert (enclosed) ● a calculator.…
Chemical equilibrium is the point at which the concentrations of reactants and products do not change with time. It would appear as if the reaction has stopped, but in fact, the rates of the forward and reverse reactions are equal, causing the reactants and products to be created at the same rate. This can be expressed mathematically in the form of the equilibrium constant. The following is the general equation for a reversible chemical reaction:…
1) If we increase the molarity of NaOH from 0.1M to 0.2M, it will actually take less number of drops in order to change the color of the solution. This is because the more concentrated a substance is, less of the substance is needed to cause an equilibrium shift.…