The first step in the industrial recovery of zinc from the zinc sulfide ore is roasting,...
The first step in the industrial recovery of zinc from the zinc
sulfide ore is roasting, that is, the conversion of ZnS to ZnO by
heating:
2ZnS(s) + 3O2(g) → 3ZnO(s) +
2SO2(g) ∆H = –879 kJ/mol
Calculate the heat evolved (in kJ) per gram of ZnS roasted.
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The first step in the industrial recovery of zinc from the zinc
sulfide ore is roasting,...
3) The first step in the industrial recovery of zinc from the zinc sulfide ore is...
3) The first step in the industrial recovery of zinc from the zinc sulfide ore is roasting that is conversion of ZnS to ZnO by heating: 2ZNS(s)+ 302[g)2ZnO(s) + 2S02(g) AH--879 KJ/mol Calculate the heat evolved (in KJ) per gram of ZnS roasted. (3 points) 4) Given the thermochemical equations: (3 points) AHO-188 KJ/mol AH-768 KJ/mol Br2)+ F2g) 2BrF(g) Br2)+3F2(g) 2BrF3(g) Calculate the AHm for the reaction BrF(g)+ F2(g) BrF3(g)
6:25 of zinc ster is the industry Me from so is the conversion of Zns to...
6:25 of zinc ster is the industry Me from so is the conversion of Zns to zno by heating : nas) + 30 (9) -> 2205) SOC) - AH = -879 Kolmoj Calculate the heat evolved (in kJ) per gram of ZnS reasted.
Zinc sulfide reacts with oxygen according to the reaction: 2ZnS(s)+3O2(g)→2ZnO(s)+2SO2(g) A reaction mixture initially contains 4.8...
Zinc sulfide reacts with oxygen according to the reaction: 2ZnS(s)+3O2(g)→2ZnO(s)+2SO2(g) A reaction mixture initially contains 4.8 mol ZnS and 7.5 molO2. Part A Once the reaction has occurred as completely as possible, what amount (in moles) of the excess reactant is left?
Zinc sulfide reacts with oxygen according to the reaction: 2ZnS(s)+3O2(g)→2ZnO(s)+2SO2(g) A reaction mixture initially contains 4.6...
Zinc sulfide reacts with oxygen according to the reaction: 2ZnS(s)+3O2(g)→2ZnO(s)+2SO2(g) A reaction mixture initially contains 4.6 mol ZnS and 9.4 mol O2. Once the reaction has occurred as completely as possible, what amount (in moles) of the excess reactant remains? Express your answer using two significant figures.
Chemistry
The "roasting" of 48.7 g of ZnS at constant pressure gives off 220. kJ of heat. Calculate the DH for this reaction.2ZnS(s) + 3O2(g) ® 2ZnO(s) + 2SO2(g)A.) -110 kJ/mol rxnB.) -293 kJ/mol rxnC.) -440. kJ/mol rxnD.) -881 kJ/mol rxnE.) +440. kJ/mol rxn
There are two steps in the extraction of copper metal from chalcocite, a copper ore. In...
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)...
1. Many important metals occur as sulfide, arsenide, and antimonide minerals, especially in the Sudbury mineral...
1. Many important metals occur as sulfide, arsenide, and antimonide minerals, especially in the Sudbury mineral complex. The first step in processing these ores involves “roasting” the ore in air to produce the metal or metal oxide, along with nonmetal oxides that can be serious pollutants if not trapped. Suppose that you roast 2.00 kg of the mineral marcasite, FeS2. The balanced equation for the reaction is: 4 FeS2 + 11 02 → 2 Fe2O3 + 8 SO2 (a) How...
3) The first step in the industrial recovery of zinc from the zinc sulfide ore is roasting that is conversion of ZnS to ZnO by heating: 2ZNS(s)+ 302[g)2ZnO(s) + 2S02(g) AH--879 KJ/mol Calculate the heat evolved (in KJ) per gram of ZnS roasted. (3 points) 4) Given the thermochemical equations: (3 points) AHO-188 KJ/mol AH-768 KJ/mol Br2)+ F2g) 2BrF(g) Br2)+3F2(g) 2BrF3(g) Calculate the AHm for the reaction BrF(g)+ F2(g) BrF3(g)
6:25 of zinc ster is the industry Me from so is the conversion of Zns to zno by heating : nas) + 30 (9) -> 2205) SOC) - AH = -879 Kolmoj Calculate the heat evolved (in kJ) per gram of ZnS reasted.
1. Many important metals occur as sulfide, arsenide, and antimonide minerals, especially in the Sudbury mineral complex. The first step in processing these ores involves “roasting” the ore in air to produce the metal or metal oxide, along with nonmetal oxides that can be serious pollutants if not trapped. Suppose that you roast 2.00 kg of the mineral marcasite, FeS2. The balanced equation for the reaction is: 4 FeS2 + 11 02 → 2 Fe2O3 + 8 SO2 (a) How...
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