Like many metals, aluminum reacts with a halogen to give a metal halide. 2 Al(s) + 3 Br2(ℓ) n Al2Br6(s) What mass of Br2, in grams, is required for complete reaction with 2.56 g of Al? What mass of white, solid Al2Br6 is expected? Methane, CH4, burns in oxygen. What are the products of the reaction? Write the balanced equation for the reaction. What mass of O2, in grams, is required for complete combustion of 25.5 g of methane? What is the total mass of products expected from the combustion of 25.5 g of methane? The metals industry was a major source of air pollution years ago. One common process involved “roasting” metal sulfides in the air: 2 PbS(s) + 3 O2(g) !’"#$%&⎯⎯) 2 PbO(s) + 2 SO2(g) If 2.50 mol of PbS is heated in air, what amount of O2 is required for complete reaction? What amounts of PbO and SO2 are expected? Iron ore is converted to iron metal in a reaction with carbon. 2 Fe2O3(s) + 3 C(s) ’!"#$%&⎯⎯) 4 Fe(s) + 3 CO2(g) If 6.2 mol of Fe2O3(s) is used, what amount of C(s) is needed, and what amounts of Fe and CO2 are produced?
- Like many metals, aluminum reacts with a halogen to give a metal halide. 2 Al(s) + 3 Br2(ℓ) n Al2Br6(s)
What mass of Br2, in grams, is required for complete reaction with 2.56 g of Al? What mass of white, solid Al2Br6 is expected?
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- Methane, CH4, burns in oxygen.
- What are the products of the reaction?
- Write the balanced equation for the reaction.
- What mass of O2, in grams, is required for complete combustion of 25.5 g of methane?
- What is the total mass of products expected from the combustion of 25.5 g of methane?
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- The metals industry was a major source of air pollution years ago. One common process involved “roasting” metal sulfides in the air:
2 PbS(s) + 3 O2(g) !’"#$%&⎯⎯) 2 PbO(s) + 2 SO2(g)
If 2.50 mol of PbS is heated in air, what amount of O2 is required for complete reaction? What amounts of PbO and SO2 are expected?
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- Iron ore is converted to iron metal in a reaction with carbon.
2 Fe2O3(s) + 3 C(s) ’!"#$%&⎯⎯) 4 Fe(s) + 3 CO2(g)
If 6.2 mol of Fe2O3(s) is used, what amount of C(s) is needed, and what amounts of Fe and CO2 are produced?
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- Sodium sulfide, Na2S, is used in the leather industry to remove hair from hides. The Na2S is made by the reaction
Na2SO4(s) + 4 C(s) !’"#$%&⎯⎯) Na2S(s) + 4 CO(g)
Suppose you mix 15 g of Na2SO4 and 7.5 g of C. Which is the limiting reactant? What mass of Na2S is produced?
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- Ammonia gas can be prepared by the reaction of a metal oxide such as calcium oxide with ammonium chloride.
CaO(s) + 2 NH4Cl(s) ’!"#$%&⎯⎯) 2 NH3(g) + H2O(g) + CaCl2(s)
If 112 g of CaO and 224 g of NH4Cl are mixed, what is the limiting reactant, and what mass of NH3 can be produced?
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- The compound SF6 is made by burning sulfur in an atmosphere of fluorine. The balanced equation is
S8(s) + 24 F2(g) !’"#$%&⎯⎯) 8 SF6(g)
Starting with a mixture of 1.6 mol of sulfur, S8, and 35 mol of F2, (a) Which is the limiting reagent?
- What amount of SF6 is produced?
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- Disulfur dichloride, S2Cl2, is used to vulcanize rubber. It can be made by treating molten sulfur with gaseous chlorine:
S8(ℓ) + 4 Cl2(g) ’!"#$%&⎯⎯) 4 S2Cl2(ℓ)
Starting with a mixture of 32.0 g of sulfur and 71.0 g of Cl2, (a) Which is the limiting reactant?
- What is the theoretical yield of S2Cl2?
- What mass of the excess reactant remains when the reaction is completed?
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- Ammonia gas can be prepared by the following reaction:
CaO(s) + 2 NH4Cl(s) ’!"#$%&⎯⎯) 2 NH3(g) + H2O(g) + CaCl2(s)
If 112 g of CaO and 224 g of NH4Cl are mixed, the theoretical yield of NH3 is 68.0 g (Study Question 12). If only 16.3 g of NH3 is actually obtained, what is its percent yield?
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- The deep blue compound Cu(NH3)4SO4 is made by the reaction of copper(II) sulfate and ammonia.
CuSO4(aq) + 4 NH3(aq) !’"#$%&⎯⎯) Cu(NH3)4SO4(aq)
(a) If you use 10.0 g of CuSO4 and excess NH3, what is the theoretical yield of Cu(NH3)4SO4? (b) If you isolate 12.6 g of Cu(NH3)4SO4, what is the percent yield of Cu(NH3)4SO4?
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