OWLY2 Online teacngagenow.com/ilm/takeAssignment/takeCovalentActivity.do?locatorcignH Image result for sp...M Gmail* MapsE Attendance March. MClassroomClipboar.nami...OYouTubeWM RealCleansdep,aptera What is the balanced equation for this reaction?O FeCl2 (aq) + Na,S(aq)FeS(s) +2 NaCl(aq)O IrCl2 (aq) + Naz S(aq) IrS(s) +2 NaCl(aq)O FeCl2 (aq) + Na, SO, (aq)FeSO, (aq) +2 NaCI(ag)O FeCl2 (aq) +Na, S(aq) FeS(s) + NaCl(aq)CorrectThe balanced equation for this reaction is:FeCl2 (aq) + Naz S(aq) FeS(s) +2 NaCl(aq)b If you combine 27 g each of NazS and FeCl2, what is the limiting reactant?O NazSO FeCl2SubmitNot VisitedTry Another Version10 item attempts remainingduf7

According to the Law of conservation of mass " all atoms of different elements must be equal on both…

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Fundamentals Of Analytical Chemistry

9th Edition

ISBN:9781285640686

Author:Skoog

Publisher:Skoog

Chapter22: Bulk Electrolysis: Electrogravimetry And Coulometry

Section: Chapter Questions

Problem 22.20QAP

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World production of chromite (FeCr₂O₄), the main ore ofchromium, was 1.5107metric tons in 2003. To isolate chro-mium, a mixture of chromite and sodium carbonate is heated inair to form sodium chromate, iron(III) oxide, and carbon diox-ide. The sodium chromate is dissolved in water, and this solutionis acidified with sulfuric acid to produce the less soluble sodiumdichromate. The sodium dichromate is filtered out and reduced with carbon to produce chromium(III) oxide, sodium carbonate,and carbon monoxide. The chromium(III) oxide is then reduced to chromium with aluminum metal. (a) Write balanced equations for each step. (b) What mass of chromium (in kg) could be pre-pared from the 2003 world production of chromite?
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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.
Gaseous F2reacts with water to form HF and O₂,. In NaOH solution, F₂, forms F⁻, water, and oxygen difluoride (OF₂,), ahighly toxic gas and powerful oxidizing agent. The OF₂, reacts with excess OH, forming O₂,, water, and F⁻. (a) For each reac-tion, write a balanced equation, give the oxidation state of O inall compounds, and identify the oxidizing and reducing agents.(b) Draw a Lewis structure for OF₂,, and predict its shape.
A 0.4740-g pesticide sample was decomposed by wet ashing and then diluted to 200.0 mL in a volumetric flask. The analysis was completed by treating aliquots of this solution as indicated. Calculate the percentage of copper in the sample.
matter eith constant composition in its structure is classified as?
give balance equation showing oxidation of H2S into S.
What is the oxidation state for KMnO4? Please show or explain calculation
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
The key reaction (unbalanced) in the manufacture of syn-thetic cryolite for aluminum electrolysis is HF(g)+ Al(OH)₃(s) +NaOH(aq) →Na₃AlF₆(aq) +H₂O(l) Assuming a 95.6% yield of dried, crystallized product, whatmass (in kg) of cryolite can be obtained from the reaction of 365 kg of Al(OH)₃, 1.20 m3of 50.0% by mass aqueous NaOH (d=1.53 g/mL), and 265 m³ of gaseous HF at 305 kPa and 91.5°C? (Assume that the ideal gas law holds.)
A sample of impure KI weighing 0.600 g is dissolved in water, the solution acidified, and 25.00 mL of 0.0400 M KIO3 (an excess ) is added. The iodate is reduced to I2 and the iodide is oxidized to I, The I2 is boiled off, the solution cooled, and an excess of pure KI is added to react with the unused KIO3. The I2 produced is titrated with 40.38 mL of 0.1053 N thiosulfate. Write the equations for the reactions which occurred and calculate the percentage of KI in the sample.
The lead(IV) oxide used in car batteries is prepared by coat-ing the electrode plate with PbO and then oxidizing it to leaddioxide (PbO₂). Despite its name, PbO₂ has a nonstoichiometricratio of lead to oxygen of about 1/1.98. In fact, the holes in the PbO₂ crystal structure due to missing O atoms are responsiblefor the oxide’s conductivity. (a) What is the mole % of O miss-ing from the PbO₂ structure? (b) What is the molar mass of the nonstoichiometric compound?

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