A 6.14-g sample containing only Mn2(SO4)3(s) and Al2(SO4)3(s) is dissolved in aqueous solution. The metal ions are precipitated as hydroxides, which are pyrolyzed in air to produce 2.24 g of a mixtureAl₂O3(s).What was the percent Mn in the original sample?%Submit Answer Incorrect. Tries 2/5 Previous TriesWhat was the percent Al in the original sample?%Submit Answer Tries 0/5

Answered: Image /qna-images/answer/7f625936-c565-497e-b785-f934c4332035.jpg

A 6.14-g sample containing only Mn2(SO4)3(s) and Al2(SO4)3(s) is dissolved in aqueous solution. The metal ions are precipitated as hydroxides, which are pyrolyzed in air to produce 2.24 g of a Al₂O3(s). What was the percent Mn in the original sample? % Submit Answer Incorrect. Tries 2/5 Previous Tries What was the percent Al in the original sample? 0/

A 6.14-g sample containing only Mn2(SO4)3(s) and Al2(SO4)3(s) is dissolved in aqueous solution. The metal ions are precipitated as hydroxides, which are pyrolyzed in air to produce 2.24 g of a Al₂O3(s). What was the percent Mn in the original sample? % Submit Answer Incorrect. Tries 2/5 Previous Tries What was the percent Al in the original sample? 0/

Chemistry for Engineering Students

4th Edition

ISBN:9781337398909

Author:Lawrence S. Brown, Tom Holme

Publisher:Lawrence S. Brown, Tom Holme

Chapter4: Stoichiometry

Section: Chapter Questions

Problem 4.98PAE

See similar textbooks

Similar questions

In the laboratory you combine 0.125 g of nickel with CO and isolate 0.364 g of Ni(CO)x. What is the value of x?
Write the balanced NET ionic equation for the reaction when aqueous CS3PO4 and aqueous AGNO3 are mixed in solution to form solid A93PO4 and aqueous CSNO3. O4- 2. 2+ 3+ 4+ + 1 3 4 7 8 9. O4 O8 (s) (1) (g) (aq) + Ag Cs Reset • x H2O Delete 3. 3.
Macmillan Learning A powder contains FeSO4 · 7 H₂O (molar mass = 278.01 g/mol), among other components. A 3.665 g sample of the powder was dissolved in HNO3 and heated to convert all iron to Fe³+. The addition of NH3 precipitated Fe₂O3 xH₂O, which was subsequently ignited to produce 0.342 g Fe₂O3. . What was the mass of FeSO4 · 7 H₂O in the 3.665 g sample? mass of FeSO4.7H₂O: 0.76 Incorrect g
Please answer as soon as you can. A 3.375 g sample of impure Al2(CO3)3 (MM = 233.9898) decomposed with HCl; the liberated CO2 (MM = 44.01) was collected on calcium oxide and found to weigh 3.601 g. What is the percentage of Al (MM = 26.98) in the sample?
How many moles of nitric acid, HNO3, are needed to react with 2.56 moles of Cu in the following reaction? - 3 Cu + 8 HNO3 --> 3 Cu (NO3)2 + 2 NO + H2O
Given the reaction below, how many grams of KI are needed to produce 2.0 g of the yellow solid PbI. 2KI + Pb(NO) :-Pbl, (s) + 2KNO3 1. 00.72 2. 02.70 3. 00.54 4. 0144
1- Consider the reaction at room temperature of 6.7 g of a pure sample of bismuth (III) sulfide, which is reacted with 75 mL of 2.5 M nitric acid solution, forming elemental sulfur, nitrogen monoxide, nitrate bismuth(III) and water. Indicate which statement is correct: Alternatives: A. The limiting reagent is nitric acid, and 0.56 g of nitrogen monoxide is formed. B. The limiting reagent is bismuth(III) sulfide, and 0.29 L of nitrogen monoxide is formed under standard conditions of pressure and temperature. C. 0.39 g of nitrogen monoxide is formed and the excess reactant is nitric acid. D. The reactant in excess is nitric acid and 0.58 L of nitrogen monoxide is formed under standard conditions of pressure and temperature. E. The limiting reagent is bismuth(III) sulfide and 0.29 L of water is formed.
CALCULATION PROBLEMS Gravimetric Problems To determine the amount of iron in a dietary supplement, a random sample of 15 tablets weighing a total of 20.505 g was ground into a fine powder. A 3.116-g sample of the powdered tablets was dissolved and treated to precipitate the iron as Fe(OH)3. The precipitate was collected, rinsed, and ignited to a constant weight as Fe,O3, yielding 0.355 g. Report the iron content of the dietary supplement as g FeSO4 7H,0 per tablet.
A K2SO4•Al2(SO4)3•24H2O preparation is tested for its purity by converting first to Al(OH)3 then finally to Al2O3. If you start with a 1.2391 g K2SO4•Al2(SO4)3•24H2O and obtained 0.1357 g Al2O3(A). What can you say about the obtained purity value? Is it acceptable?(B). Which is a better choice of precipitate for the quantitative analysis of K2SO4•Al2(SO4)3•24H2O, Al(OH)3 or Al2O3? Explain
4. A mixture of 3.00 g of Bi2O3 and 0.500 g C are used to produce bismuth and CO in the reaction Bi2O3 + 3 C → 2Bi + 3 CO Determine the limiting reagent and the excess reagent. 50/ 00% DI 20/ C L G
a. What mass of AgI can be produced from a 0.512-g sample that assays 20.1% AlI3?b. Precipitates used in the gravimetric determination of uranium include Na2U2O7 (634.0 g/mol), (UO2)2P2O7 (714.0 g/mol), and V2O5 · 2UO3 (753.9 g/ mol). Which of these weighing forms provides the greatest mass of precipitate from a given quantity of uranium?
A) Determine the ionic formula of one Cr+6, 4 oxygen atoms (polyatomic ion with a charge of -8) and 2H+ ions. B) Find the molar mass of one mole of the compound in part A. C) The Michigan standard for the maximum permissible level of Cr+6 in ground water is 0.10 mg/L. You take 1.00 Liter of ground water and discover that there is 0.15 mg of Cr+6 present. Convert 0.15mg of Chromium (the +6 charge does NOT change the molar mass) to moles of Cr. D) How many formula units of H2CrO4 are in the number of moles of Cr+6 you calculated in part C? r