Need help with this lab practical, specifically how to calculate everything for

Question

Need help with this lab practical, specifically how to calculate everything for the calculation part

Stoichiometry of Redox Reaction A Lab Practical chemistry-201 Write a rk in this re sheet Page 1 of 6 Names Do not talk to anyone during this practical. If you need clarification see instructor. Put you name on this lab sheet Show all work to receive full credit Record your data based on the precision of the instrument and use correct significant figures Wear safety goggles and gloves Wear hand protection when handling hot glassware. Wash hands immediately if any KMno4 gets on your hands When a new oxidation-reduction reaction is found, an important goal is to determine the identities of the products in the reaction. If one of the products is known, then the second product can be identified by first determining the stoichiometric ratio of the reactants and then balancing electrons to determine the oxidation state of the atoms in the second product. By balancing the redox reaction the identity of the second product may be deduced The reaction you wi nvestigate today is equation (1) HONH3 (aq) 3+, (aq) 2+ Reaction (Acidic) Unbalanced Redox Reaction 2+, (aq) ent and Che als HONH Litmus papers 3-125 mL Elm Flask 25 mL Buret 1-25 mL Grad cylinder KMno. Fe2(SO4)s 10-mL Vol pipet/bulb 3 M HCI DI water Wax pencil Hot plate For 10 students (three trials): 600ml HONH Procedure: Prepare three identical samples by following the following directions Make sure you have all the glassware necessary to perform this experiment through its entirety. Clean all glassware before the experiment to avoid contamination of your experiment. Note that the concentrations of hydroxylamine [A], iron(III) sulfate [B], and potassium permanganate [C] will be given to you when you begin your experiment. Prepare a sample by pipetting 10.00 mL of a -CAL Maqueous solution of hydroxylamine into a 125 mL Erlenmeyer flask Add 25 mL of the IBl M aqueous solution of iron (III) sulfate by using the graduated cylinder by the reagent bottle or through the repipetor. This amount represents an excess of iron Add approximately 1 mL of 3 M HCl to the iron(III) sulfate and test the fy that it is acidic. The dropper may be calibrated or you can count 20 drops. (20 drops 1 mL) solution with litmus to ver Boil the solution for five minutes over a hot plate and then let the solution coo n an ice bath. Wear hand protectors when removing the hot solution from the hot plate During this cooling period, add 1 drop of hydroxylamine solution into a clean test tube. Add three drops of the iron (III) sulfate solution to this and heat briefly by setting the test tube on a hot plate or in hot water. Add a few drops of potassium permanganate to the test tube and write your observation. This is the result you should observe when iron(II) ions are oxidized to ron(III) in your titration If you have time, work on the supplemental questions at the end of this lob practical or use the concentration of the hydroxylamine to calculate the moles of hydroxylamine used in this experiment obtain approximately 50 mL of KMno4 and use this solution to fill the Buret at your lab station. Fill a 25-mL buret with standardized ICL MKMno4 solution. Record the initial volume of the buret. use your knowledge of titration to set up the buret for this procedure without assistance from your instructor. If you are not comfortable in the titration technique, look at the previous labs performed this semester that utilized titration technique Titrate the cooled sample with KMno4 solution until the first permanent color change occurs (as observed in Step 4) in the mixture. A good strategy is to use one sample to determi ne the approximate amount of KMno4 required to reach the endpoint of the solution the endpoint can also be observed in this first trial. In general, the solution goes from pale yellowish orange to a deep orange violet. Use the second and third sample to carefully determine the exact volume of KMno4 required t reach the endpoint. 8. Record the final volume for your titration in the data sheet Rinse all equipment with deionized water and clean your work area

Explanation / Answer

Titration data is needed for other calculations.

5. mole ratio of Fe2+/nydrolxylamine reacted = 2/2 = 1

6.

i. Oxidation of state of N in hydroxylamine,

a. -1

ii. The nitrogen oxidation state in product,

c. +1

iii. The nitrogen oxide product would be,

d. N2O

7. Balanced equation,

2NH3OH+ + 2Fe3+ --> 2Fe2+ + N2O + H2O + 6H+

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