Chalcopyrite (CuFeSa), is an important source of copper. A typical chalcopyrite ore contains about0.75% Cu. What volume of sulfur dioxide at 25°Cand 1 atm pressure is produced when one boxcarload (4x 10^3 cu.ft} of chalcopyrite ore (density = 2.6 g/cu.cm) is roasted? Assume all the sulfur in the ore is converted to SO2 and no other %3D source of sulfur is present

Chalcopyrite (CuFeSa), is an important source of copper. A typical chalcopyrite ore contains about0.75% Cu. What volume of sulfur dioxide at 25°Cand 1 atm pressure is produced when one boxcarload (4x 10^3 cu.ft} of chalcopyrite ore (density = 2.6 g/cu.cm) is roasted? Assume all the sulfur in the ore is converted to SO2 and no other %3D source of sulfur is present

Introductory Chemistry: A Foundation

9th Edition

ISBN:9781337399425

Author:Steven S. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Donald J. DeCoste

Chapter15: Solutions

Section: Chapter Questions

Problem 10CR

See similar textbooks

Similar questions

In the presence of nitric acid, UO2+ undergoes a redox process. It is converted to UO22+ and nitric oxide (NO) gas is produced according to the following unbalanced equation: H+(aq)+NO3(aq)+UO2+(aq)NO(g)+UO22+(aq)+H2O(l) If 2.55 102 mL NO(g) is isolated at 29C and 1.5 atm, what amount (moles) of UO2+ was used in the reaction? (Hint: Balance the reaction by the oxidation states method.)
To prepare a very dilute solution of K2Cr2O7 (294.18 g/mol), 0.661 g of K2Cr2O7 was transferred to a 250.0-mL volumetric flask and adding water to the mark. A sample of this solution of volume 1.000 mL was then transferred to a 500.0-mL volumetric flask and diluted to the mark with water. Subsequently, 10.0 mL of the diluted solution was transferred to a 250.0-mL flask and diluted to the mark with water. What is the final concentration of K2Cr2O7 in this last solution?
One method of removing CO2(g) from a spacecraft is to allow the CO2 to react with LiOH. 2LiOH(s)+CO2(g)→Li2CO3(s)+H2O(l) How many liters of CO2(g) at 23.6 ∘C and 1.00 barr can be removed per 9 kg of LiOH consumed?
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 sample of ultrapure silicon was reacted with excess oxidizing yielding SiO2. After properfiltration and drying, the precipitate weighed 3.1754 g. If ultrapure silicon is 99.98% Si, what massof sample was used?
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?
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%)
Write a balanced equation for this process. Liquid potassium (k) is reacted with solid aluminium oxide (Al2O3) and potassium oxide(K2O) dust is produced.
A 235.2-g sample of ground water is analyzed for calcium. The Ca2+ in the sample is first precipitated and filtered-off as NH4CaPO4·7H2O. This precipitate is dried and heated, releasing water and ammonia to yield anhydrous calcium pyrophosphate (Ca2P2O7). The mass of Ca2P2O7 obtained is 0.0234 g.Give the calcium content of the ground water in parts per million (to three significant figures).
What is the balanced equation for water is driven from copper sulfate pentahydtate,CuS04*5H2O,with heat?
A 244.5-g sample of ground water is analyzed for calcium. The Ca2+ in the sample is first precipitated and filtered-off as NH4CaPO4.7H20. This precipitate is dried and heated, releasing water and ammonia to yield anhydrous calcium pyrophosphate (CaP2O7). The mass of CaP2O, obtained is 0.0419 g. Give the calcium content of the ground water in parts per million (to three significant figures).
The gravimetric analysis of a 11.432-gram sample of silver ore yields 4.918 grams of silver iodide [MW=234.77 g/mole]. Determine the percent by weight of silver metal [At.Wt. = 107.868 g/mole] in the ore.