Reference no: EM13129477
1. For the NEW bottle of hydrogen peroxide, record and calculate the following:
(a) Initial burette reading of potassium permanganate used in each titration (mL) and concentration:
(b) The volume of potassium permanganate required to titrate each 10.00 mL portion of the new hydrogen peroxide (mL): (record all three trials' data)
(c) Calculate the number of moles of the H2O2 in the 10.00 mL sample in every titration from the volume of KMnO4 used and the stoichiometry of the reaction.
(d) Take the average of the two closest values you found in step (c).
(e) Use the average from step (d) to calculate the molarity of the H2O2.
(f) Calculate the % by mass (mass) of H2O2 in the original sample. Assume the density is 1.00 g/mL for the NEW H2O2. (MW of H2O2 is 34.01 amu)
2. Repeat the calculations for the OLD bottle of H2O2:
(a) Initial burette reading of potassium permanganate used in each titration (mL) and concentration:
(b) The volume of potassium permanganate required to titrate each 10.00 mL portion of the old hydrogen peroxide (mL):(record all three trials's data)
(c) Calculate the number of moles of the H2O2 in the 10.00 mL sample in every titration from the volume of KMnO4 used and the stoichiometry of the reaction.
(d) Take the average of the two closest values you found in step (c).
(e) Use the average from step (d) to calculate the molarity of the H₂O₂.
(f) Calculate the % by mass of H2O2 in the original sample. Assume the density is 1.00 g/mL for the OLD H2O2.(MW of H2O2 is 34.01 amu)
3. Commercial hydrogen peroxide contains small amounts of organic compounds that are added to stabilize it. If these compounds react with permanganate, how would this affect your results in terms of the % by mass of H2O2?
my data was: KMnO4 added to new peroxide: 20ml to reach the end point
18.1ml
18.05ml
KMnO4 added to old peroxide: 16ml to reach end point
molarity for KMnO4 is .2M 13ml to reach end point
12.65ml to reach end point
the chemical reaction given to use for calculation is:
2[MnO4-]aq + 6[H+]aq + 5[H2O2]aq ---> 5[O2]g + 2[Mn(2+)]aq + 8[H2O]l
|
Property costs in the company accounting records
: The property included land appraised at $87,500, land improvements appraised at $35,000, and a building appraised at $52,500. What should be the allocation of this property's costs in the company's accounting records?
|
|
Standard quantity allowed for units production
: The standard quantity allowed for the units produced was 6,500 pounds, the standard price was $2.50 per pound, and the materials quantity variance was $375 favorable. Each unit uses 1 pound of materials. How many units were actually produced?
|
|
Nitration of methyl benzoate
: In the nitration of methyl benzoate, why do you wash the crystals with water followed by an ice-cold methanol washing? What is the purpose of pouring the reaction mixture over ice?
|
|
Describe the various approaches required by current gaap
: describe the various approaches required by current GAAP standards for reporting changes in accounting principles. Discuss how these approaches may be impacted by the adoption of new IFRS standards.
|
|
Calculate the number of moles of the h2o2
: Calculate the number of moles of the H2O2 in the 10.00 mL sample in every titration from the volume of KMnO4 used and the stoichiometry of the reaction.
|
|
What is partial pressure of cl2 in the equilibrium mixture
: At 373 K, Keq = 2.39 for the following reaction: SO2Cl2(g) = SO2(g) + Cl2(g) In an equilibrium mixture of the three gases, the partial pressures of SO2Cl2 and SO2 are 3.31 atm and 1.59 atm, respectively.
|
|
Which of the following statements is not accurate
: Which of the following statements is not accurate?
|
|
To what temperature must the gas be heated
: A sample of nitrogen gas is contained in a piston with a freely moving cylinder. At 0 C, the volume of the gas is 307 mL. To what temperature must the gas be heated
|
|
What is the balance in the investment
: What is the balance in the Investment in Harrison account found in the financial records of Puckett as of December 31?
|