FeCl2•4H20(aq) + H2C2O4(aq)→ Fe C204 • 2H2O(s) +2H2O(/) + 2HCI(aq) A sample of FeCl2 • 4H2O with mass equal to 3.76 g of reacts with an excess of oxalic acid to form 2.88 g of Fe C204 • 2H2O is produced. Calculate the percent yield of the product. Use the following molar masses: FeCl2 • 4H2O -198.81g/mol Fe C204• 2H20 - 179.89 g/mol.

FeCl2•4H20(aq) + H2C2O4(aq)→ Fe C204 • 2H2O(s) +2H2O(/) + 2HCI(aq) A sample of FeCl2 • 4H2O with mass equal to 3.76 g of reacts with an excess of oxalic acid to form 2.88 g of Fe C204 • 2H2O is produced. Calculate the percent yield of the product. Use the following molar masses: FeCl2 • 4H2O -198.81g/mol Fe C204• 2H20 - 179.89 g/mol.

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

16.792 g of Ba(OH)2 (171.342 g.mol') is weighed out and carefully dissolved to make a 500.00cm³ solution. A 25.00 cm³ 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 HN3. Ba(OH)2(aq) + 2HNO3(aq) Ba(NO3)2(aq) +2H2O(1) The moles of Ba(OH)2 transferred to the beaker is: 1.96 x 10-3 mol 5.21 x 10-3 mol 4.90 x 10-2 mol 1.96 x 10-1 mol O 3.92 x 103 mol None of the above
In the reaction Zn(s) +Cu2+(aq) Zn2*(aq) + Cu(s), O Cu2*(aq) is the oxidizing agent and Zn(s) is the reducing agent. O Cu2*(aq) is the bxidizing agent and Zn2*(aq) is the reducing agent. O Cu(s) is the oxidizing agent and Zn(s) is the reducing agent. O Zn(s) is the oxidizing agent and Cu2*(aq) is the reducing agent. e Textbook and Media Hint Save for Later pe here to search
The chemical reaction occurring during the discharge of a lead storage battery can be represented by the following equation. How many grams of PBSO, produced if 80 g of Pb, 90 g of PbO2, and 500 ml of 0.68 M solution of H,sO, is used? Pb(s) + PbO;(s) +2 H;SO.(aq) – 2 PbSO.(s) + 2 H;0(1I)
16.792 g of Ba(OH)2 (171.342 g.mol-1) is weighed out and carefully dissolved to make a 500.00cm3 solution. A 25.00 cm3 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(NO3)2(aq) + 2H2O(l) The moles of Ba(OH)2 transferred to the beaker is:
Consider the following reaction: Zn(s) + Cu2+(aq) ⟶ Cu(s) + Zn2+(aq) Which reactant is oxidized?
To determine the amount of iron in a dietary supplement, a random sample of 23 tablets weighing a total of 847 g was ground into a fine powder. A 0.5046 g sample of the powdered tablets was dissolved and treated to precipitate the iron as Fe(OH)3(106.95g/mol). The precipitate was collected, rinsed, and ignited to a constant weight as Fe2O3.(159.69g/mol) yielding 0.5445 grams. Report the iron content of the dietary supplement as g FeSO4.7H₂O (277.91g/mol) per tablet. Unit should not be written in the box.
A sample with a mass of 1.340 g was dissolved in water, releasing chlorine ions. The aqueous solution was treated with access AgNO3(aq), the AgCl precipitate collected and weighted. Its mass was 2.709 g. What percentage by mass was the original sample? Make sure to use the correct number of significant figures in your answer.
A 2.37 g sample of a mixture of FeCl2 and Fe(NO3)2 is treated with excess AgNO3(aq). The precipitate is filtered off, dried and weighed. The dried precipitate weighs 4.05 g. What is the percentage by mass of FeCl2 in the original mixture? Your answer must be accurate to two sig figs.
McQuarrie · Rock Gallogly A 0.3146 g sample of a míxture of NaCI(s) and KBr(s) was dissolved in water. The resulting solution required 37.40 ml. of 0.08765 M AGNO, (aq) to precipitate the CI (aq) and Br (aq) as AgCI(s) and AgBr(s). Calculate the mass percentage of NaCI(s) in the mixture. mass percentage: % NaCI
In an electrolysis of a solution with sodium chloride NaCl(aq), sodium hydroxide is formed NaOH(aq), chlorine gas Cl2(g), and hydrogen gas H2(g), after the reaction equation: 2NaCl(aq) + 2H2O(l) → 2NaOH(aq) + Cl2 (g) + H2(g) a) An electrolysis is a redox reaction. What substance is oxidized, and what substance is reduced in the electrolysis of the solution with sodium chloride NaCl(aq)? Base your answer by showing to change in oxidation figures. b) Use the table at the back of the task set and set up two half-reactions describing what is happening on the anode and cathode of this electrolysis.
A 1.53 g sample of a mixture of FeCl2 and Fe(NO3)2 is treated with excess AgNO3(aq). The precipitate is filtered off, dried and weighed. The dried precipitate weighs 1.92 g. What is the percentage by mass of FeCl2 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): N, 14.01 O, 16.00 Cl, 35.45 Fe, 55.85 Ag, 107.9
A stock solution of potassium permanganate (KMnO4) was prepared by dissolving 17.1 g KMnO4 with DI H2Oin a 100.00-mL volumetric flask and diluting to the calibration mark. Determine the molarity of the solution.