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CMI Experiment =
Empirical Formula of a Compound
Pre-Lab Procedure (Volume Cutter Lab)
AlM
What is the empirical formula for glucose, C6H12O6?
Manganese(II) acetate is made by combining manganese and acetic acid. The resulting solution is placed in a container and heated. Where does the manganese acetate compound precipitate?
Why must we use the method of calculating molar mass to determine the empirical formula? (1 pt)
Name one of the main safety concerns with working with 6M HCl. (1 pt)
Calculate the molar mass of C6H12O6. (3 pts)
Calculate the number of moles of HCl in 6M HCl. (2 pts) Show work.
A 3.24g of titanium reacts with 8g of oxygen to form the titanium oxide. What is the empirical formula for the resulting oxide? (2 pts) Show work.

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03:08

Lab report: Denzoic Acid

At Vrk#ecFaclb;TUnInSAlthough the purpose of this experiment was to investigate the recrystallization of Denzoic Acid, there were several graphical errors in the data. These errors affected the accuracy of the melting point values. Please refer to the attached document for detailed instructions on how to interpret the experimental data.

Denzoic Acid:Geometric crystallizationData and Determinationpoints-Molecular Ratio and HopuieanalyticalCemeaL MP LL AF demaibBenzoic8469 55 k TDhite 122.3*4241.201.27 CcincolorlcsWaterExperimental melting point (provide a range): 121-123Â°CTheoretical Recovery: 4.47 mol (1H6O2 / 22vâ‚¬)Actual Recovery: 55.0 g and 87.4%Percent Recovery: 62.2%

Calculations:Theoretical Recovery: 5.1a 31141 c9lyc7h6 92 24ITx/075; C14 772Y1 VePercent Recovery: 21.56(1_nolfdL%y Percen 4 37.17: 4.0744625,5184l,2

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08:37

Post-Lab Questions 3: THE EMPIRICAL FORMULA OF A COMPOUNDConsider the following deviations from the experimental procedure: Explain how each of these deviations specifically affects the mass of the copper recorded (increase/decrease/stay the same)? Note: single word, not an explanation.1. The student did not wait for the blue color to disappear but continued and collected the precipitated copper by vacuum filtration.2. Copper remained in the beaker during the transfer to the Buchner funnel.3. The copper on the filter paper was not dry when the final mass was recorded.

In an experiment, a student isolated 6.356 g of pure copper from an initial sample of 9.902 g of a copper chloride compound. Determine the empirical formula of this compound (show your work).

Answer:How many grams of carbon are there in 835.801 g of formaldehyde; CH2O, which is 40.09 u carbon by mass (show your work)?

Your doctor has diagnosed you as being anemic and has recommended that you take an iron…

01:44

Experiment 19 Prelaboratory Assignment: Aspirin Synthesis and AnalysisName: Desk No: Date: Lab Sec:Procedure, Part A:In the experiment, 2.00 g of salicylic acid (molar mass 138.12 g/mol) reacts with an experimental excess amount of acetic anhydride. Calculate the theoretical yield of acetylsalicylic acid (molar mass 180.2 g/mol) for this synthesis.

After completing the experimental procedure, a mass of 1.78 g of acetylsalicylic acid was obtained. What is the actual yield for its synthesis? Express the yield with the correct number of significant figures.

Experimental Procedure, Part B:Recrystallizing Medium:Explain how to perform the recrystallization of the product obtained in Part A.

05:11

Laboratory DateSlctlumlExperiment 9 – Post-lab Questions Mclhinol (CH OH)en Muluced Uee Feaclicri of carbon muxnuide (CO) with hydrogen (H2). The talaa chrinical nuctionCuei 4 – CH OH()~upot /i olcurkan mtonotick icniclcduu4 gofhydogen. Which rcucbint Anetmitinp inls?What is the theoretical yield?InahancA Vic comnketimactnnof excess TelEcn will rcusin?IroniII) oxid (Fe2O3) can con enco ncFdhaik- etu wth carhon (C). Where the Moucl Aclun Ulutue (CueIkhlmn c lctn mecticn2R;Fash 3 CO(h)punnia molcs &l onumatidc6CuCEcuHow’ HiLII ` Hlokt ol cuntun Ar necdcu mecbn ehoexactly widl ual e with ILO Airxunt of cithctHow many nioles offiFOn will ploduccui?How many moles of curbrn diotide will prouceui?Fnt

01:53

POST-LAB QUESTIONSCalculate the total mass percent of the copper compound.The total mass % of the copper compound is 0.0259%.Calculate the total mass percent of the cobalt compound.The total mass % of the cobalt compound is 0.013g.Calculate the total mass percent of the chromium compound.The total mass % of the chromium compound is 0.0179%.Assuming you had correctly followed the experimental procedure, what could be a possible reason why the combined percentage of the compounds decreased during the extraction and isolation procedures?In addition, state how this reason could possibly be mitigated.One possible reason for the decrease in the combined percentage of the compounds during the extraction and isolation procedures is that some of the compounds may have been lost or left behind during the process. This could be mitigated by ensuring that all equipment and containers are properly cleaned and that the extraction and isolation procedures are carried out carefully and accur…

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