2. A 1.1324 g sample of an iron ore is dissolved in acid. The iron is oxidized to a +3 state and is precipitated as Fe₂O3.xH₂O. The precipate is filtered, washed and ignited to Fe₂O3 (159.69 g mol-¹). 0.5394 g Fe₂O3 is produced. The reaction is 2Fe³+ Fe₂O3(s). Calculate the percentage of Fe3O4 (231.54 g mol-¹) in the sample. Fe (55.847 g mol-¹)

2. A 1.1324 g sample of an iron ore is dissolved in acid. The iron is oxidized to a +3 state and is precipitated as Fe₂O3.xH₂O. The precipate is filtered, washed and ignited to Fe₂O3 (159.69 g mol-¹). 0.5394 g Fe₂O3 is produced. The reaction is 2Fe³+ Fe₂O3(s). Calculate the percentage of Fe3O4 (231.54 g mol-¹) in the sample. Fe (55.847 g mol-¹)

Chemistry

10th Edition

ISBN:9781305957404

Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Chapter1: Chemical Foundations

Section: Chapter Questions

Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...

See similar textbooks

Similar questions

How many grams of Cu(OH)2 will precipitate when excess KOH solution is added to 41.0 mL of 0.618 M CuBr2 solution? CuBr2(aq) + 2KOH(aq) Cu(OH)2(s) + 2KBr(aq)g?
How many grams of Ag₂CO3 will precipitate when excess Na₂CO3 solution is added to 49.0 mL of 0.590 M AgNO3 solution? 2AgNO3(aq) + Na2CO3(aq) → Ag2 CO3(s) + 2NaNO3(aq) g
A solution of NaCl(aq) is added slowly to a solution of lead nitrate, Pb(NO3)₂(aq), until no further precipitation occurs. The precipitate is collected by filtration, dried, and weighed. A total of 10.67 g PbCl₂ (s) is obtained from 200.0 mL of the original solution. Calculate the molarity of the Pb(NO3)₂(aq) solution. concentration: M
16.792 g of Ba(OH)2 (171.342 g.mol') is weighed out and carefully dissolved to make a 500.00cm solution. A 25.00 cm of this solution is pipette then transfer into a 100.00 mL volumetric flask, filling up to the mark with water. A 40.00 mL sample of this diluted solution is then reacted with a 0.753 M solution of HNO3. Ba(OH)2(aq) + 2HNO3(aq) → Ba(N03)2(aq) + 2H2O(1) The concentration of Ba(OH)2 in the 100.00 cm3 volumetric flask is: O 1.96 x 103 M O 5.21 x 10-3 m O 4.90 x 10 2M O 1.96 x 101 M O 3.92 x 103 M O None of the above
Solid copper can be produced by passing gaseous ammonia over solid copper (II) oxide at high temperatures, according to the following reaction. NH3 (g) + CuO (s) → N2 (g) + Cu (s) + H2O (g) Balance the reaction.
How many grams of magnesium phosphate, Mg3(PO4)2, would you need if you were required to make 270.0 mL of a magnesium phosphate solution with a concentration of 0.170 mol L-1? Molar masses: Mg3(PO4)2 = 262.9 g mol-1 1 L = 1000 mL What is the concentration of PO43- ions in the 0.170 mol L-1 solution of magnesium phosphate?
You are making 750 mL of a 0.7 M Ca(OH)2 solution. How many moles of Ca(OH)2 will be added? How many grams of Ca(OH)2 will be massed out in a weigh boat?
Give the net ionic equation for the reaction (if any) that occurs when aqueous solutions of K 2S and Fe(NO 3) 2 are mixed.
Excess Na2SO4(aq) is added to a 4.41×102 mL sample of industrial waste containing Ba2+ ions. If 55.5 g of BaSO4(s) are precipitated from the reaction, what was the molar concentration of Ba2+ in the original sample?
A 0.9 g sample of a mixture of KCl and MgCl2 is treated with excess AgNO3(aq). If 2.37 grams of AgCl(s) are obtained, then what is the percentage by mass of KCl in the original mixture? Your answer must be accurate to two significant digits. Keep several extra digits in your calculations and round off only at the end. Do not include the percent sign (%) as part of your answer. Molar masses (in g mol−1): KCl, 74.55 MgCl2, 95.21 AgCl, 143.35
Suppose that a solution prepared by dissolving 0.554 g of MgCl2 in about 30 mL of water is mixed with a solution that contains excess K2CO3 dissolved in about 30 mL of water. What is the theoretical yield (in grams) of MgCO3 in the precipitation reaction that occurs?
Lead ions can be precipitated from solution with KC1 according to the following reaction: Pb²+ (aq) + 2 KCl(aq) → PbCl₂(s) + 2 K+ (aq) When 28.8 g KCl is added to a solution containing 25.5 g Pb²+, a PbCl₂ precipitate forms. The precipitate is filtered and dried and found to have a mass of 29.6 g. Part A Determine the limiting reactant. KCI Pb²+ Submit Part B m = Determine the theoretical yield of PbCl₂. Submit Part C Request Answer ΨΕ ΑΣΦ Submit Request Answer Determine the percent yield for the reaction. ΨΕ ΑΣΦ Request Answer BE ? ? % g