1. Chalcopyrite(CuFeS2) is an abundant copper mineral that can be converted to elemental copper. How much Cu is there in 1.00 kg CuFeS2?
2. Combustion analysis of an unknown compound indicated that it is 92.23% C and 7.82% H. The mass spectrum indicated the molar mass is 78g/mol. What is the molecular formula of this unknown compound?
3. Ascorbic acid also known as Vitamin C, is an organic compound containing C,H, and O. The combustion of a 28.1 g sample of ascorbic acid produces 42.1g CO2 and 11.5 g H2O. Determine the empirical and molecular formula of ascorbic acid. The molar mass is 176g/mol.
1. Chalcopyrite(CuFeS2) is an abundant copper mineral that can be converted to elemental copper. How much...
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
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.
Ascorbic acid also known as Vitamin C, is an organic compound containing C, H and O. The combustion of a 28.1 g sample of ascorbic acid produces 42.1 g CO2 and 11.5 g H2O. Determine the empirical and molecular formula of ascorbic acid. The molar mass is 176 g/mol.
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...
19 Question (1 point) See page 302 "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 Cu S in...
6. A certain compound has the following elemental composition: C, H, O, N. In a combustion analysis, 3.895 g of it was combusted to produce 9.087 g of CO2 and 3.411 g H20. Separate analysis determined that it is 12.38% N, and its molar mass is 226.4 g/mol. Determine its empirical and molecular formula.
6. A certain compound has the following elemental composition: C, H, O, N. In a combustion analysis, 3.895 g of it was combusted to produce 9.087...
A 13.56 gram sample of copper is heated in the presence of excess bromine. A metal bromide is formed with a mass of 30.60 g Determine the empirical formula of the metal bromide. ter the elements in the order C B empirical formula A 5.267 gram sample of an organic compound containing C, H and O is analyzed by combustion analysis and 13.29 grams of CO2 and 2.332 grams of H20 are produced In a separate experiment, the molar mass...
1) Calculate the number of moles of Cl atoms in 3.01×1024 formula units of magnesium chloride, MgCl2. Express your answer numerically in moles. 2) In the gaseous state, chlorine exists as a diatomic molecule Cl2 (Molar mass = 70.9 g/mol). Calculate the number of moles of chlorine present in 100 g of chlorine gas. Express the quantity in moles to three significant figures. 3) Sodium hydroxide, NaOH, is a strong base that is used in industrial synthesis and processes such as...
1) How many moles of water, H2O, contain 2.0×1022 molecules of water? Express the quantity in moles to two significant figures. Moles of water = ___________ mol 2) In the gaseous state, chlorine exists as a diatomic molecule Cl2 (Molar mass = 70.9 g/mol). Calculate the number of moles of chlorine present in 140 g of chlorine gas. Express the quantity in moles to three significant figures. Moles of chlorine gas = ___________ mol 3) Sodium hydroxide, NaOH, is a strong...
1) Calculate the number of moles of Cl atoms in 3.01×1024 formula units of magnesium chloride, MgCl2. Express your answer numerically in moles. 2) In the gaseous state, chlorine exists as a diatomic molecule Cl2 (Molar mass = 70.9 g/mol). Calculate the number of moles of chlorine present in 100 g of chlorine gas. Express the quantity in moles to three significant figures. 3) Sodium hydroxide, NaOH, is a strong base that is used in industrial synthesis and processes such...