Differential Kinetics And Error Analysis

To conduct this experiment I first measured the combined mass of a filter paper and a 250 mL beaker. I then removed the filter paper from the beaker and decanted 100 mL of clear saturated PbCl2 and 20 mL of .5M K2CrO4. I had to be careful when handling the PbCl2 and the K2CrO4 because lead and chromate compounds are toxic.After I heated the mixture to its boiling point and let it rest for five minutes. I had to be careful when handling the beaker because a hot beaker looks the same as

Solutions of 6M H2SO4, 6M NH3, 6M HCl, 6M NaOH, and 1.0 M of NaCl, 1M Fe(NO3)3, 1M NiSO4, 1M AgNO3, 1M KSCN, 1M Ba(NO3)2, and 1M Cu(NO3)2 were given in separate test tubes. The color of possible precipitates, ions, acid-base behaviour, odor and solubility rules were conducted and were reported in Table 1. The key information about a mixture of two solutions was

The purpose of the experiment was to find the absorbance value and T% of cobalt (II) nitrate solutions at various wavelengths. Using Beer’s law to determine the concentration of an unknown cobalt (II) nitrate solution with the %T and A values of the known Cobalt (II) nitrate concentrations.

7. The initial and final volume along with the grams of the analyte was recorded on the data sheet and the amount of KMnO4 for each flask was calculated. Calculations and recordings of the mass percent of iron in the unknowns were finished.

Keq for all trials. The following table shows the keq values for all trials as well as the average. Calculations …for finding the concentration of KSCN after the reaction ran to completion (trial 2) KSCN Concentration (M)= (initial concentration (M)x volume KSCN used (M))/(total volume (L))=M KSCN KSCN Concentration (M)= 0.002 M x 0.008 L= (0.000016 moles)/(0.0016 L)=0.001 M KSCN …for finding the concentration of KSCN at equilibrium y=503.88x+0.007 y=absorbance at equilibrium 0.52=503.88x+0.007 x=0.001018   Discussion The objective of this experiment was to find the equilibrium constant for the complex ion formation of Fe and SCN.

However, adsorption process using bentonite much longer than composites. In addition, the separation of bentonite from the solution requires filter. If using bentonite-Fe3O4 composite, separation without filter. The separation can be using permanent magnet. Treatment of acid mine drainage synthetic using bentonite-Fe3O4 composite (2:1) having final concentration of Fe2+, Cu2+, Zn2+ and Mn2+ were 5.66, 14.09, 15.34 and 21.75 mg/L, respectively. Therefore, it is recommended to use the bentonite-Fe3O4 composite (2:1) to treatment acid mine drainage. The adsorption efficiency for all adsorbent increases in the order Mn2+< Zn2+< Cu2+< Fe2+. The same result in the adsorption process using bentonite blended limestone while adsorption efficiency to the Mn2+ of the smallest compared to other metal ions such as Fe, Co, Cr, Cu, Pb and Zn [22]. Another study that bentonite adsorption affinity order of the metal ions from acid mine drainage was Zn<Ni

As I researched about my dream job, I realized how math concepts are used. One well known concept is decimals.

After a week in a dark cabinet, the solid was placed through a vacuum filter to get rid of the excess amount of water through it. When it was finished filtering, the KTOF was put into a Petri dish and weighed to find the actual yield of the reactant that was used in the experiment. The dry weight experiment was used to determine how much water was used to create the solid into KTOF. In order to calculate the amount of water that was used to make the KTOF, evaporating dishes were used to dry out the KTOF. The experiment used a specific amount of KTOF that was weighed on the top loading balance and then placed into a mass of K3[Fe(C2O4)] mortar to crush the solids.

The answer to the question of “What is the empirical formula of this substance containing zinc and chlorine?” Simply put, the answer is ZnCl2. This is what the empirical formula is because when the mass of each substance is converted into number of atoms, the ratio of Zinc to Chlorine is about 2:1 for almost every trial conducted. See Figure 1. Equations 1 and 2 demonstrate how the conversions were performed and how moles/ molecular weights of each substance were incorporated in the calculations.

John. A. Avers conducted a purification experiment of Zirconium via ion exchange to determine the percentage of recovery of the element. John A. Avers used various resins to determine which would obtain the highest purification of zirconium compared to other ion exchange resins and the extraction of the element will be conducted by using Zirconium from ores. Some of the resins used consisted of rare earths, beryllium, titanium and iron. John A. Ayers took zirconium ore’s and broke them down by using concentrated sulfuric acid. 8 Once the zirconium ore was broken down, the soluble zirconium was then converted to its nitrate form, Zr(NO3)4. The zirconium nitrate is then passed through a column containing a resin. The hydrogen form of Amberlite I.R.-100 was used as the

First we added 4 mL of HNO3 into a beaker. After the substance dissolved, distilled water was added until the beaker the beaker was half full. The mixture was then stirred into the distilled water. Add 30 mL of NaOH into the solution, and stir. The solution was then heated slow. As the product was heating slowly it was stirred. A thermoter was placed on a ringstand and clamp and then placed inside the solution.The solution was heated until 61 degrees celsius. The beaker was then removed from the heat and left to settle. 200 mL of distilled water was placed inside a 400 mL beaker and put on the heater. When the CuO settled for 10 minutes, the solution was then placed inside of a funnel. After the solution is drained, the copper is then washed away with the distilled water. The soultion was tested with a litmius paper. 15 mL of 6.0 mL of H2So4 into the solution. Next the Zinc must be added, then observe the reaction. Then add 10 mL of 6 M Hcl to the Cu. Pour out the Hcl, then add water to the copper and rinse. Then get a beaker and add Cu to water and apply heat.

The chemistry lab is a place where I’ve made some interesting discoveries about the microscopic interaction of particles. Yet, percent error calculations in lab reports may prove otherwise. After completion of a lab, we are able to calculate the theoretical yield of an experiment based on the amounts used in the chemical reactions. However, this yield rarely comes close to the amount actually produced by the experiment. This has made me think, what is the point of performing these labs if we can never get close to the expected amount? Are the theories behind the stoichiometry of chemical reactions inaccurate?

From the testing and results several major trends and relationships were discovered. The first observation, which supports the hypothesis, is the relationship between concentration of reactants and reaction rate. As concentration increased, the reaction rate also increased in direct proportion. This was shown by the results because when the concentrations doubled, from 0.1M and 0.125M to

Kinetics of chemical reactions is how fast a reaction occurs and determining how the presence of reactants affects reaction rates. In this experiment the rate of reaction for Fe+3 and I- is determined. Because the rate of chemical reactions relates directly to concentration of reactants, the rate law is used to find the rate constant, and calculated with specified temperatures.

The equation of the line in run 1 between the two points is y – y1 = m(x – x1)