Description attached is a pdf worksheet that must be completed please change the pdf to a word document so you can write your answers in the provided space
Description The Challenge for this weeks worksheet is to use the numbers obtained by a student to complete the “Identification of unknown Metal Carbonate” pages in the lab manual (pg 65-66) then submit a pdf copy to the Gradescope page. Deadline Friday Oct 9 at 5 pm. A video of the experimental basics is athttps://www.youtube.com/watch?v=V6jP1Jt59Xc To prepare for the experiment you need to read the lab manual pg 59-63, paying specific attention to how the mass percent of CO2 is determined for a compound. You will need to calculate Mass percent of CO2 for each of the Carbonates listed in table 9-3. Remember that if you have a “hydrate” as shown on page 60, you must use the entire Molar mass including the number of water molecules to find the correct theoretical percent CO2. The goal is to use the numbers generated by a student to find your unknown. The scene: A student weighed a beaker and test tube, mass was determined as 129.02 g. Some Lithium Carbonate was added and now the mass was 130.22 g. Acid was added to the test tube and the total mass before reaction was 139.73 g. The acid was dumped into the beaker (see video for observations) and now the entire assembly weighed 139.01 g.It is up to you to use these numbers to make sure you know how to do the calculations and get the correct mass percent for Lithium Carbonate. Next the student took an unknown carbonate and performed the same steps, repeating for accuracy. Items weighed Trial 1 Trial 2 Beaker + test tube 136.14 g 134.75 g Beaker + test tube +carbonate 137.25g 136.04 g Beaker + test tube +carbonate + acid 146.87 g 148.22 g Mass of assembly after reaction 146.69 g 147.99 g The calculations and questions to answer: Use this information to fill in the tables on pg 65, in table 9-1 you should be able to obtain the correct mass percent for Lithium Carbonate. This allows you to make sure you understand the process. Fill in the data table 9-2 for your unknown carbonate. Find the Mass % of CO2 in the unknown carbonate, compare to table 9-3 ( that you filled out in the preparation for this lab) and name which unknown you have. Find the % error in your results (question 1) remembering that the error is an absolute value. Watch the video again to think about sources of error. List 3, and decide which could have the greatest impact on your results. Apply what you learned when calculating % CO2 in a carbonate, and calculate % Cl in Group II metal chlorides. It is the same procedure, but now you are considering chlorine instead of CO2. If you do not remember what Group II is, use your textbook to refresh your memory. Remember to show calculations for all sections.
Description 1. Fill in the Data table Table 1. Raw data for the calibration curve portion of the measurement of an equilibrium constant experiment Solution # Concentration (M) Absorbance 1 0.00E+00 0 2 6.18E-05 0.154 3 1.03E-04 0.22 4 1.44E-04 0.352 5 2.06E-04 0.514 Table 2. Raw and processed Data for the determination of the equilibrium constant portion of the measurement of an equilibrium constant experiment Concentration of Fe3+ (M) Concentration of SCN- (M) Test Solution Test solution Test solution Initial Volume SCN- (mL) Initial Concentration SCN- (M) Initial Volume Fe3+ (mL) Initial concentration Fe3+ (M) Absorbance Equilibrium concentration Fe(SCN)2+ (M) Reacted Concentration of Fe3+ (M) Reacted Concentration of SCN- (M) Equilibrium Concentration of Fe3+ (M) Equilibrium Concentration of SCN- (M) Equilibrium Constant Average Equilibrium Constant Standard Deviation of Equilibrium Constant 2. Complete the results section that in found in the lab manual attached below pages 205-206. The experiment is pages 195-206. The raw data in excel is also attached below. Please include a picture of any graphs as well as on excel because my excel is old. 3. include 1-5 sentences that briefly summarize the procedure and what information was obtained ? Example: – ____ g (or mL) of Reagent A were reacted with _____ g (or mL) of Reagent B until a precipitate formed/gas evolved/color change occurred. Observations were made and data were collected. Table 1 represents _____. Table 2 represents _____. Figure 1 represents _____. Figure 2 represents ____. 4. Complete the Discussion: In your discussion section address the following questions: ? How does your equilibrium compare with the rest of the class? ? Is there much class variation in the results? ? What does the calculated equilibrium constant tell you about the equilibrium position of the reaction you studied? Does the reaction favor reactants or products? ? Compared with the class is your mean and standard deviation similar? Why or why not? 5. Also include a conclusion, Example: ? Restate the purpose of the experiment ? How did you attempt to meet the purpose? ? Was the purpose met? ? Restate the anticipated outcome. Was the actual outcome close to the anticipated outcome? ? Why or why not? What errors did you specifically experience in this experiment? – Distance-learning format of the class is not an error ? What are some future improvements to this experiment? – “Updating the lab manual”, “clear/better instructions on how to perform calculations”, “instructor not explaining the lab procedure”, “do not make the class a distance-learning course”, etc. are NOT future improvements Please let me know if you have any questions!
Description Please answer the following lab questions and show work along with the step and the solutions. Use the data below to answer the questions. Thank you in advance mass NaHCO3: 7.1904 moles NaHCO3: 0.0856 mol liters NaHCO3: 50 mL
Description All the directions are in the file converting between units is an important part of any science. Below is a table with measurements that are common in chemistry. In the table, useful equalities are given.
Description I also have a video and more instructions I will link after! Watch the “Lab 2 – Green Synthesis of Camphor Demo Video” on Blackboard, and use the information and data below to complete your lab report. Fill in the spaces provided. DATA Mass of Isoborneol: 0.3855 g Mass of crude (impure) camphor: 0.4122 g Mass of pure camphor produced (after sublimation): 0.2036 g Infrared Spectra IR Spectrum and spectral data table of Isoborneol Use the spectrum above to complete the table below. Select the important wavenumbers and the associated assignments and interpretation: Wavenumber (cm-1) Assignment Interpretation R Spectrum and spectral data table of Camphor Use the spectrum above to complete the table below. Select the important wavenumbers and the associated assignments and interpretation: Wavenumber (cm-1) Assignment Interpretation Questions In the green synthesis of camphor, a 0.3885 g isoborneol sample was treated with excess sodium hopchlorite (NaOCl). What would be the theoretical yield of camphor? Show work. Calculate the percent yield of the camphor in the reaction? Show work (Hint: %yield = experimental yieldtheoretical yield x 100%). Predict the products of the following reactions: (a) (b) In the experiment, both the starting isoborneol compound and camphor are white solids. What evidence leads you to conclude that these two solids are in fact different compounds and that the unreacted starting material was not isolated? (Hint: compare the infrared spectra of both isoborneol and camphor). Give one reason why the mass of the crude product is larger than the theoretical yield. Describe some green features of this experiment.
Description List the starting materials, solvent, reagent, temperature range (low, room temperature, or high) and products formed: How long did it take to finish the reaction? List any important IR peaks (If no noteworthy peaks, answer “none”). Are there any IR peaks NOT PRESENT that indicate the product was formed? (Hint: think about the functional groups of the starting material and the product) List the 1H NMR peaks. List the peak number, chemical shift, multiplicity (splitting pattern), and the integration. List the 13C NMR peaks. List the peak number and the chemical shift. What is the intermediate of this reaction? What is the leaving group (Hint: think about the mechanism)? What is the nucleophile? 2-methyl2-propanol +HCl =2-chloro2-methylpropane
