The copper mineral chalcocite (Cu2S) can be converted to copper by heating in air:
Cu2S (s) + O2 (g) -----------> 2Cu (s) + SO2 (g)
How many grams of SO2 is produced?
Cu2S(s) + O2(g) -------> 2Cu(s) + SO2(g)
From the balanced equation, 159.1 g Cu2S or 1 mol Cu2S gives 1 mol of SO2 or 64 g SO2.
Hence mass of SO2= 64 g
The copper mineral chalcocite (Cu2S) can be converted to copper by heating in air: Cu2S (s)...
"Native," or elemental copper can be found in nature, but most copper is mined as oxide or sulfide minerals. Chalcopyrite (CuFeS2) is one copper mineral that can be converted to elemental copper in a series of chemical steps. Reacting chalcopyrite with oxygen at high temperature produces a mixture of copper sulfide and iron oxide. The iron oxide is separated from CuS by reaction with sand (SiO2). CuS is converted to Cu2S in the process and the Cu2S is burned in...
Chalocopyrite (CuFeS2) is an abundant copper mineral that can be converted into elemental copper. What is the percentage composition of CuFeS2? How many grams of iodine are in 45.325 g of calcium iodate, Ca(IO3)2.
See page 302 19 Question (1 point) *Native," or elemental copper can be found in nature, but most copper is mined as oxide or sulfide minerals. Chalcopyrite (CuFeS2) is one copper mineral that can be converted to elemental copper in a series of chemical steps. Reacting chalcopyrite with oxygen at high temperature produces a mixture of copper sulfide and iron oxide. The iron oxide is separated from CuS by reaction with sand (SiO2). CuS is converted to Cu2S in the...
suppose an ore sample contains 10.0 impurity in addition to a mixture of cus and cu2s. Heating 100.0g of the mixture produces 76.2g of copper metal with a purity of 90.4%. What is the weight percent of cus of the ore? The percent of cu2s? Copper metal can be prepared by roasting copper ore, which can contain cuprite (CuzS) and copper(II) sulfide. Cu,S(s) + O2(g) + 2 Cu(s) + SO2(E) CuS(s) + O2(g) + Cu(s) + S02 (8) Suppose an...
Copper was one of the first metals used by humans because it can be recovered from several copper minerals including cuprite (Cu2O), chalcocite (Cu2S), and malachite [Cu2CO3(OH)2]. Balance the following reactions for converting these minerals into copper metal: (A) Cu2O(s) + C(s) → Cu(s) + CO2(g) (B) Cu2O(s) + Cu2S(s) → Cu(s) + SO2(g) (C) Cu2CO3(OH)2(s) + C(s) → Cu(s) + CO2(g) + H2O(g)
There are two steps in the extraction of copper metal from chalcocite, a copper ore. In the first step, copper(I) sulfide and oxygen react to form copper(I) oxide and sulfur dioxide: 2Cu2S (s) + 3O2 (g) → 2Cu2O (s) + 2SO2 (g) In the second step, copper(I) oxide and carbon react to form copper and carbon monoxide: Cu2O (s) + C (s) → 2Cu (s) + CO (g) Write the net chemical equation for the production of copper from copper(I)...
When copper reacts with sulfur at high temperature, copper(I) sulfide is formed. 2Cu(s) + S(s) → Cu2S(s) If the mass of the Cu2S formed is 1.17 g, what mass of copper should have reacted?
Chalcopyrite (CuFeS2) is an abundant copper mineral that can be converted into elemental copper through the four step process below. Part 1 Calculate the mass of Cu in g from 8.40 kg CuFeS2. ________g Part 2 Calculate the mass of CuFeS2 needed in g to produce 300.0 g Cu if the yield for the conversion process is 82%. _________g
4. Consider the following reactions: Cu20 + Cu2S Cu+SO2 250 kg of copper (I) oxide is heated with 129 kg of copper () sulfide. A) Determine the limiting reagent [T/I - 3, C-1] B) How much copper is recovered in (g)? [T/I -2, C-1] C) How many grams of the excess reactant remains [T/I 3, C-1] Show all your work Cu7O 143.1 CurS 15
Small quantities of oxygen can be prepared in the laboratory by heating potassium chlorate, KClO3(s) . The equation for the reaction is 2KClO3⟶2KCl+3O2 Calculate how many grams of O2(g) can be produced from heating 70.4 g KClO3(s) STRATEGY: Convert the mass of KClO3 to moles. Convert the number of moles of KClO3 to the number of moles of O2 . Convert the number of moles of O2 to grams. Step 1: 70.4 g KClO3 is equal to 0.574 mol KClO3...