An iron blast furnace produces pig iron of composition 94.2% Fe, 3.5% C, 1.5% Si, 0.8% burden of blast furnace consists of the following materials. Limestone is pure CaCO, ar converted to CaO that makes up 36% of the slag. The analysis of exit gas is given as 269 13% CO, and 61% N,; assume no loss of iron in slag. Rational Analysis wt% Material Fe,03 SiO2 Al,03 MnO
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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?Blast furnace produces pig iron of composition Fe 94%, Si2%, Mn 0.5% and C 3.5% by reduction smelting of iron ore, coke and limestone. The analysis is as follows: Iron ore : Fe,0, 78%, SiO, 8%, Alz0, 5%, MnO 2% H20 7% Coke : 86% C and 10% S and 4% Al,0,; Amount is 600 Kg per ton of pig iron Limestone : pure Caco, to produce a slag of 45% Cao Calculate: a) Amount of ore/ton of pig iron b) % of total Si 0z and of Mn0 reduced in the furnace c) Amount of slag/ton of pig iron and its % composition.The maximum solid solubility of carbon in ferrite occurs at 0.022 wt% C and 727 ° C, the eutectoid composition is 0.76 wt% C, the maximum solid solubility of carbon in austenite occurs at 2.14 wt% C and 1147 ° C, and the cementite composition is 6.7 wt% C. For 2122 g of a 3.2134 wt% C steel at 726 ° C, what will be the mass of carbon present as part of a compound?(a) 67.9 g(b) 74.2 g(c) 58.7 g(d) 83.5 g
- A basic lining is given to a furnace by using:(a) Calcined dolomite(b) Copper sulphate(c) Haematite(d) SilicaAluminum 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…(i) Name the method of refining to obtain low boiling metal like mercury, (ii) What is the role of pine oil in froth floatation process? (iii) Reduction of metal oxide to metal becomes easier if the metal obtained is in liquid state. Why?
- A 0.8965g ore sample is dissolved in nitric acid and then filtered. The aluminum is present in solution as AP". The solution is made basic with ammonium hydroxide, NH,OH, and the aluminum hydroxide, Al(OH)» (FW 78.004), precipitates. This gel is filtered in a porous glass crucible, rinsed with dilute ammonium hydroxide, ignited, cooled in a desiccator, and weighed. The resulting alumina, Al;O; (FW 101.94), weighed 0.1605 g. Why is the solution filtered after acid dissolution? Why rinse with ammonium hydroxide solution? What chemical transformation takes place during ignition? (Show the balanced chemical equation) • Why use a desiccator during cooling? Calculate the weight percent Al (AW 26.9815) in the sample. Al(OH)) -> Al;O, + H0A sample of feldspar weighing 1.500g is decomposed, and eventually there is obtained a mixture of KCl and NaCl weighing 0.1801 g. These chlorides are dissolved in H2O, a 50-mL pipetful of 0.08333 N AGNO3 is added, and the precipitate is filtered off. The filtrate requires 16.47 mL of 0.1000N KCNS, with ferric alum as indicator. Calculate the percentage of K2O in the silicate.A series of reactions is carried out on the alloy (A) formed of two metals, as in the following scheme : Amount of ppt. (B) +H2SO4(aq) +NAOH(ag) +NaOHçaq) Decreases and a Alloy Aqueous solution Ppt. (B) white green ppt. remains What are the two metals forming alloy (A)?.. a) Copper and aluminum b) Copper and iron c) Iron and aluminum d) Iron and lead.
- A 0.8965 g sample is dissolved in HNO; and filtered. The aluminum is present in solution as AP. The solution is made basic with ammonium hydroxide, NH.OH, and the aluminum hydroxide, Al(OH): (FW 78.004), precipitates. This gel is filtered in a porous glass crucible, rinsed with dilute ammonium hydroxide, ignited, cooled in a desiccator, and weighed. The resulting alumina, Al:O: (FW 101.94), weighed 0.1605 g. Why is the solution filtered after acid dissolution? • Why rinse with ammonium hydroxide solution? • What chemical transformation takes place during ignition? (Show the balanced chemical equation) Why use a desiccator during cooling? • Calculate the weight percent Al (AW 26.9815) in the sample.detailed and concise info about the PROCESSES OF MINERAL ORIGIN/ ORIGIN and GEOGRAPHICAL DISTRIBUTION of Carbonates, nitrates, and boratesA 600.0 mg sample consisting of only CaC2O4and Mg C2O4is heated at 500oC converting the two salts to CaCO3and MgCO3. The sample weighs 465.0 mg. If the sample had been heated at 900oC where the products are CaO and MgO, what would the mixture of oxides weigh? Write in a padpaper and show the clear and complete solution