A quantity of ore consist of 90% (by weight) chalcopyrite mineral with a composition of CuFeS2. The rest is inert quartz, SiO2. The ore is roasted by heating it in oxygen at 800oC. This process converts the ore into Fe2O3 and CuO. The two oxides are separated from each other and from the quartz using density differences and subsequently the oxides are reduced to the metal using carbon. A total of 349 kg of iron metal is obtained.
What is the mass of sulfur dioxide set free? kg
What is the mass of carbon dioxide set free? kg
What is the mass of quartz tailings produced? kg
Answers need to be within 1% accurate.
Molar masses: Fe: 55.8, Cu: 63.5, S: 32, O: 16, C: 12, Si: 28 [g/mol]
Hint There is a similar problem on wikis.lib.ncsu.edu, see http://wikis.lib.ncsu.edu/index.php/CH_101/Exercises_3 under example 6.
A quantity of ore consist of 90% (by weight) chalcopyrite mineral with a composition of CuFeS2. The rest is inert quartz, SiO2. The ore is roasted by heating it in oxygen at 800oC. This process converts the ore into Fe2O3 and CuO. The two oxides are separated from each other and from the quartz using density differences and subsequently the oxides are reduced to the metal using carbon. A total of 349 kg of iron metal is obtained.
What is the mass of sulfur dioxide set free? kg
What is the mass of carbon dioxide set free? kg
What is the mass of quartz tailings produced? kg
Answers need to be within 1% accurate.
Molar masses: Fe: 55.8, Cu: 63.5, S: 32, O: 16, C: 12, Si: 28 [g/mol]
Hint There is a similar problem on wikis.lib.ncsu.edu, see http://wikis.lib.ncsu.edu/index.php/CH_101/Exercises_3 under example 6.
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