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- In the metallurgy of antimony, the pure metal is recovered from the sulfide ore by...
1. In the metallurgy of antimony, the pure metal is recovered from the sulfide ore by the following reaction: SbS(s) + 3Fe (s) 2 Sb(s) + 3FeS () AH-125 kJ Calculate AS un for this reaction at 25°C and 1 atm. 2. Predict the sign of AS., for each of the following reactions. Write "positive" or "negative". a. PCI (8) PCI (1) + Cl2 (g) b. CH. (g) +20, (g) CO2 (g) + 2 H20 (1) c. Mg(s) + Cl2...
) sulfide reacts with nitric acid according to the reaction below: 5. Antimony(III) sulfide reacts w Sb2S3(s) + 10 HNO3(aq) → Sb2Os(5) a. Calculate the theoretical yield in sulfide reacts with 0.579 mol nitric acid. O HNO3(aq) Sb Os(s) + 10 NO(g) + 3 S(s) + 5 H200 clical yield (in grams) of each product when 32.1 g of antimony(1) 321 gs bz63 x 1 mol sbg 82 x mol sbag Molsb2S₃ 0.519 HNO3 x 01 Slezs - Imolsberg Omo...
Pure titanium metal can be extracted from Ti02 which is found as and ore in the Earth's crust. How many kg of pure titanium can be recovered from 200.0 pounds of this ore?(1lb=454g)
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)
Heating a 6.600 g sample of an ore containing a metal sulfide, in the presence of excess oxygen, produces 1.450 L of dry SO, measured at 50.0 °C and 752.5 Torr. Calculate the percent by mass of sulfur in the ore. Assume that all sulfur in the sample was converted to SO. S(s) + O(g) → SO(g)
Heating a 6.568 g sample of an ore containing a metal sulfide, in the presence of excess oxygen, produces 1.466 L of dry SO, measured at 46.8 °C and 753.8 Torr. Calculate the percent by mass of sulfur in the ore. Assume that all sulfur in the sample was converted to SO. S(s) + O(g) → SO(g)
1 - Mass balance with reaction a) A certain amount of Pennsylvania coal, in a final analysis (by mass), has 84.36% C, 89% H2, 4.40% O2, 0.63% N2, 0.89% S and 7.83% ash (non-combustible). This coal is burned with a theoretical amount of air. Disregarding the ash content, determine the molar fractions of the products. b) The antimony is obtained by heating the tibite (Sb2S3) sprayed with iron shavings, removing the molten antimony from the bottom of the reaction tank:...
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.
I need help with part B Explanation: A mole ratio is the ratio between the amounts in moles of any two compounds involved in a chemical reaction. The mole ratio can be determined by examining the coefficients in front of formulas in a balanced chemical equation. Step 1: write the balanced chemical equation. Sb2S3(s) + 3Fe(s)→2Sb(s) +3FeS(s) Step 2: calculate the moles of Sb2S3 , Fe Moles of Fe = mass given / molar mass = ( 25 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:2 Cu_2 S(s)+3 O_2(g) rightarrow 2 Cu_2 O(s)+2 SO_2(g) In the second step, copper(I) oxide and carbon react to form copper and carbon monoxide: Cu_2 O(s)+ C(s) rightarrow 2 Cu(s)+ CO(g) Write the net chemical equation for the production of copper from copper(I) sulfide, oxygen and carbon. Be sure your...