Heating a 6.600 g sample of an ore containing a metal sulfide, in the presence of...
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)
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Heating a 6.600 g sample of an ore containing a metal sulfide, in the presence of...
Heating a 6.568 g sample of an ore containing a metal sulfide, in the presence of...
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)
suppose an ore sample contains 10.0 impurity in addition to a mixture of cus and cu2s....
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...
A manganese-containing ore is digested and chemically treated to isolate manganese as MnO2(s). Heating the MnO2...
A manganese-containing ore is digested and chemically treated to isolate manganese as MnO2(s). Heating the MnO2 at 1000 °C in air converts it entirely to Mn3O4(s). Suppose a 2.70-g ore sample yields 0.235 g of Mn3O4(s) by this process. Calculate the percent Mn in the ore sample. Calculate the percent MnO2 in the ore sample.
A manganese-containing ore is digested and chemically treated to isolate manganese as MnO2(s). Heating the MnO2 at 1000 °C in air converts it entirely to Mn3O4(s). Suppose a 2.44-g ore sample yields 0.229 g of Mn3O4(s) by this process.
A manganese-containing ore is digested and chemically treated to isolate manganese as MnO2(s). Heating the MnO2 at 1000 °C in air converts it entirely to Mn3O4(s).Suppose a 2.44-g ore sample yields 0.229 g of Mn3O4(s) by this process.Calculate the percent Mn2O3 in the ore sample.
A 21.92 gram sample of iron is heated in the presence of excess oxygen. A metal...
A 21.92 gram sample of iron is heated in the presence of excess oxygen. A metal oxide is formed with a mass of 31.33 g. Determine the empirical formula of the metal oxide. A 25.23 gram sample of chromium is heated in the presence of excess fluorine. A metal fluoride is formed with a mass of 43.67 g. Determine the empirical formula of the metal fluoride. A 7.199 gram sample of iron is heated in the presence of excess bromine....
7. A 0.250-g sample of calcium metal is heated in a 38.500-g crucible to form calcium...
7. A 0.250-g sample of calcium metal is heated in a 38.500-g crucible to form calcium oxide. The resulting crucible and product weigh 38.850 g. Refer to Example Exercise 1 and determine the empirical formula of calcium oxide. DATE DATA TABLE A Empirical Formula of Magnesium Oxide mass of crucible and cover + magnesium metal (before heating) mass of crucible and cover mass of magnesium metal mass of crucible and cover + magnesium oxide (after heating ) 0000 mass of...
5. A 0.565-8 sample of cobalt metal reacted with excess sulfur powder to give 1.027 g of cobalt sulfide
5. A 0.565-8 sample of cobalt metal reacted with excess sulfur powder to give 1.027 g of cobalt sulfide Calculate the empirical formula of the product. 6. A 0.750-g sample of tin foil was heated in air and reacted with oxygen gas to give 0.953 g of tin oxide. Calculate the empirical formula of the product. 7. (optional) A 1.000-g sample of red phosphorus powder was burned in air and reacted with oxygen gas to give 2.291 g of phosphorus oxide. Calculate...
1. A 0.750-g sample of tin metal reacts with 0.201 g of oxygen gas to form tin oxide.
1. A 0.750-g sample of tin metal reacts with 0.201 g of oxygen gas to form tin oxide. Calculate the empirical formula of the tin oxide. 2. A 0.565-g sample of cobalt metal reacts with excess sulfur to give 1.027 g of cobalt sulfide. Calculate the empirical formula of the product. 3. A 1.164-g sample of iron filings reacts with chlorine gas to give 3.384 g of iron chloride. Calculate the empirical formula of the product? 4. A 0.626-8 sample of copper oxide...
A 50.0 g sample of ore containing FeBr2 is dissolved in acid and titrated to an...
A 50.0 g sample of ore containing FeBr2 is dissolved in acid and titrated to an end point with 24.80 mL of 0.629 M Cr2O72−. The following redox reaction takes place: Cr2O72− (aq) + Fe2+ (aq) ⟶ Cr3+ (aq) + Fe3+ (aq) a. balance the reaction b. what % of the ore sample if FeBr2 (molar mass = 215.65 g/mol)
A 43.29 gram sample of cobalt is heated in the presence of excess oxygen. A metal...
A 43.29 gram sample of cobalt is heated in the presence of excess oxygen. A metal oxide is formed with a mass of 60.92 g. Determine the empirical formula of the metal oxide.
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...
7. A 0.250-g sample of calcium metal is heated in a 38.500-g crucible to form calcium oxide. The resulting crucible and product weigh 38.850 g. Refer to Example Exercise 1 and determine the empirical formula of calcium oxide. DATE DATA TABLE A Empirical Formula of Magnesium Oxide mass of crucible and cover + magnesium metal (before heating) mass of crucible and cover mass of magnesium metal mass of crucible and cover + magnesium oxide (after heating ) 0000 mass of...
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