lege-CHEM 1020 - Spring20 - NGWENDSON Activities and Due Dates > Ch 7 HWAssignment Score:42.6%ResourcesGive Up?O HintCheck AnswerKスQuestion 22 of 23 >Combining 0.256 mol Fe, O, with excess carbon produced 18.7 g Fe.Fe, 0, + 3C – 2 Fe + 3 COWhat is the actual yield of iron in moles?actual yield:molWhat is the theoretical yield of iron in moles?moltheoretical yield:What is the percent yield?terms of usecontact ushelpabout uscareersprivacy policy136.Aa59APR16DDF12DIIF11F10F9F8F720F6F5F4F3F2delete%3D&%23%24CO

The reaction is, Fe2O3 + 3 C -----> 2 Fe + 3 CO…

Answered: lege-CHEM 1020 - Spring20 - NGWENDSON…

Fundamentals Of Analytical Chemistry

9th Edition

ISBN:9781285640686

Author:Skoog

Publisher:Skoog

Chapter20: Applications Of Oxidation/reduction Titrations

Section: Chapter Questions

Problem 20.25QAP

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Done < HIIL Attempts done: 0/2 O Zn²+ O Zn O Zn²- O Zn+ What is the most common oxidation state for zinc? > AA A practice.flatworld kn Read the related chapter ? View available hints Report an error
The mercury in a 0.8142-g sample was precipitated with an excess of paraperiodic acid, H5IO6: 5 Hg 2+ + 2 H5IO6 ---> Hg5(IO6)2 (s) + 10 H + The precipitate (MW = 1448.8 g/mol) was filtered, washed free of precipitating agent, dried, and weighed, and 0.4114 g was recovered. Calculate the a) % Hg (200.6 g/mol) b) % Hg2Cl2 (472.1 g/mol)
A 0.4852g sample of an iron ore was dissolved in acid to the 3+ state, then precipitated as Fe2O3 x H2O. The pp was filtered, washed and calcined to Fe2O3, which gave a weight of 0.2481g. Calculate the Fe % in the sample.
Pls give with reason, the type and name of the reaction.
A. 1.4639 g sample of limestone was analyzed for Fe, Ca and Mg. The iron was determined as Fe2O3, yielding 0.0357 g Calcium was isolated as CaSO4, yileding a precipitate of 1.4058 g and Mg was isolated as 0. 0627 g of MgP2O7. Report the amount of Febas %w/w Fe2O3, Ca as %w/w CaO and Mg in the limestone sample as % w/w MgO
When jump-starting a car with a dead battery, the ground jumper should be attached to a remote part of the engine block. Why?
An ore containing Fe3O4 was analyzed by dissolving a 1.5419-g sample in concentrated HCl. HNO3 was then added to oxidize any Fe2+ to Fe3+. The Fe3+ was precipitated as Fe(OH)3 by adding NH3. The precipitate was collected by filtration and was finally heated yielding 0.8525 g of Fe2O3. Report the concentration of Fe3O4 in the sample as %(w/w). (Note: the final answer is said to be 53.4%)
Mo in a 0.2711g sample was precipitated giving 1.1682g of (NH4)2PO4.12 MoO3. Find the percentage Mo , P (at wt = 30.97), N=14,Mo=95.9,H=1,O=16
56g of the coal was kjeldahlized and NH3 gas evolved was absorbed in 50 ml of 0.1 N sulphuric acid. After absorption, the excess acid required 6.25 ml of 0.1 N NaOH for exact neutralization. 2.60g of the coal sample in a quantitative analysis gave 0.1755 g of BaSO4. Calculate the percentage of nitrogen and Sulphur in coal sample.
Consi‎der follo‎wing rea‎ction: HgO (s) -> Hg(l) + ½ O2 (g) Delta H = +90.7 kj/mol. Wh‎at qua‎ntity of h‎eat in kj/mol is req‎uired to prod‎uce on‎e m‎ole HgO? Wri‎te your answer wit‎hout units. Gi‎ven the fol‎lowing data 2Cl‎F(g) + O‎2(g) --> Cl2‎O(g) + F2‎O (g) De‎lta H= 167.4 kJ I 2Cl‎F3(g) + 2O‎2(g) --> Cl‎2O(g) + 3F2‎ O (g) Delta H= 341.4 kJ II 2 ‎F2(g) + O‎2(g) ---> 2F2O‎ (g) Delt‎a H= -43.4 kJ III Calc‎ulate the de‎lta H in kJ for below‎ reaction: ClF(g) + F2(g) ---> ClF3(g)
Use the following atomic masses (in g/mol):Mg = 24.31; O = 16; Ca = 40.08; C = 12.01; Na = 23; H = 1; N = 14.01; S = 32.06; Cl = 35.45; 2.) Limestone consists chiefly of mineral calcite (CaCO3). The carbonate content of 0.5413g of powdered limestone was measured by suspending the powder in water, adding 10mL of 1.392M HCl and heating to dissolve the solid and expel CO2. The excess acid required 39.96mL of 0.1004M NaOH for complete titration to a phenolphthalein end point. Find the % wt of calcite in limestone.
An impure sample of Na3PO3 weighing 0.1 g is dissolved in 35 mL of water. A solution containing 45 mL of 3% w/v HgCl2, 30 mL of 10% w/v sodium acetate, and 10 mL of glacial acetic acid is then prepared. After digesting, filtering, and rinsing the precipitate, 0.2857 g of Hg2Cl2 is obtained. Report the purity of the original sample as % w/w Na3PO3.

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