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- Fe2O3 is produced from a pyrite concentrate containing 65% by weight of pyrite (FeS2) by total oxidizing roasting according to the following reaction. 5 tons of pyrite concentrate is roasted daily (MA, g / mol; Fe: 56; S: 32; 0: 16; H: 1). 2FeS2 + 11 / 2O2 → Fe2O3 + 4SO2 How much Fe2O3 is produced in 1 day?Aluminum is the most abundant metal in the earth’s crust. It is also a common household utensilmetal. The extraction of Aluminum from its ore is expensive because the metallurgy uses a veryhigh amount of electricity. The extraction of Aluminum metal takes place in a number of steps,which may be summarized below.Step 1: Washing and mechanical processes employed to the ore to remove basic impurities.Step 2: Conversion of Aluminum ore (Bauxite) to powdered Alumina (Al2O3) by reaction withconcentrated NaOH solution.Step 3: Dissolving Alumina in molten Cryolite(Na3AlF6)Step 4: Electrolytic refining of the solution at step 2. (Diagram below) to form pure Aluminummetal.Step 5: Collecting pure molten Aluminum at the cathode, which change later to solid Aluminummetal.As you observed, many changes are taking place in different steps for the above extractionprocess. Classify them as physical or chemical change and explain why?a) Step 1 __________________________________________b) Step 2…Balance the following reaction. The charge on Cu in CuS is 2+. You may add additional phases but not components to achieve this. Show your working out. CuS(s) + HNO3(aq) --> CuSO4(s) + NO(g)
- The most important commercial ore of chromiumis chromite (FeC r 2 O 4 ). One of the steps in theprocess used to extract chromium from the ore is thereaction of chromite with coke (carbon) to produceferrochrome (FeC r 2 ).2C(s) + FeC r 2 O 4 (s) → FeC r 2 (s) + 2C O 2 (g)What mole ratio would you use to convert from molesof chromite to moles of ferrochrome?A 1.1324 g sample of magnetite ore was dissolved in concentrated HCl to give a solution that contained a mixture of Fe2+ and Fe3+. Nitric acid was added and the solution was boiled for a few minutes, which converted all of the iron to Fe3+. The Fe3+ was then precipitated as Fe2O3*xH2O by addition of NH3. After filtration and washing, the residue was ignited at a high temp to give 0.5394 g of pure Fe2O3. What is the percent Fe and the percent Fe3O4 in the sample?We have talked about in lecture about metamorphic grade, and about the difference between progradeand retrograde mineral reactions. One such possible mineral reaction is as follows:orthoclase + sillimanite + H2O = muscovite + quartz 3a: Write a balanced chemical reaction for the above minerals, given that the formula for muscovite isK2Al6Si6O20(OH)4 3b: Indicate which reaction direction (left to right, right to left) is the prograde direction, and explainwhy you think that.
- Iron corrodes to produce rust, Fe2O3, but other corrosion products that can form are Fe(O)(OH), iron oxyhydroxide, and magnetite, Fe3O4. The oxidation number for Fe in magnetite was controversial for a long time. If we assume that oxygen’s oxidation number is - 2, and Fe has a unique oxidation number, what is the oxidation number for Fe in magnetite?Sample: Commercial bleach Technical specifications:- Composition: sodium hypochlorite (NaClO) and demineralized water;- Active chlorine content: 2.00 to 2.50% (m/m);- Active ingredient: sodium hypochlorite (NaClO).- Approximate density: 1.08 g/ml;- Physical Aspect: Liquid;- Color: Colorless. Note: the active chlorine content refers to the chlorine gas produced from the following reaction:ClO¯ + Cl¯ + 2H+ ⇋ Cl₂(g) + H₂OData:M.A.: H = 1.0079 g/mol; Na = 22.989769 g/mol; S = 32.065 g/mol; I = 126.90447 g/mol; O = 15.9994 g/mol; Cl = 35.453 g/mol. Material available in the laboratory's warehouse: Reagents:Distilled water; standardized solution of sodium thiosulfate (Na₂S₂O₃), at a concentration of 0.0500 mols/L; 20% KI solution; glacial acetic acid and; starch gum (indicator). Glassware:Bechers of all sizes available on the market; 50, 100, 150, 200 and 250 ml Erlenmeyer flasks; 10.00 and 25.00 mL volumetric pipettes; 25.00 mL burette; 25.00, 50.00 and 100.0 mL volumetric flasks. Calculate…Write a balanced equation for this process. Liquid potassium (k) is reacted with solid aluminium oxide (Al2O3) and potassium oxide(K2O) dust is produced.
- 17. Consider the reaction of 0.161 g of aluminum metal with 50.0 mL of 0.235 M Co(NO₃)₂. a. Which metal, Al or Co, is more easily oxidized? b. Write the balanced chemical equation that occurs for the oxidation reaction. If no reaction occurs, simply write only NR. Be sure to include the proper phases for all species within the reaction. c. What quantity in moles of Co(NO₃)₂ do you start with? d. What quantity in moles of metal product are generated if all of the Co(NO₃)₂ is consumed? e.What quantity in moles of Al do you start with? f. What quantity in moles of metal product are generated if all of the Al is consumed? g. Which reactant is limiting? h. What mass (in grams) of metal is formed when the limiting reactant is considered?Assuming an efficiency of 39.90%,39.90%, calculate the actual yield of magnesium nitrate formed from 145.7 g145.7 g of magnesium and excess copper(II) nitrate. Mg+Cu(NO3)2⟶Mg(NO3)2+CuMagnesium Chloride is available as magnesium chloride hexahydrate in an injectable solution that supplies 1.97 mEq of magnesium per milliliter. What is the percent strength of magnesium chloride hexahydrate in this solution?