Metallic titanium and its alloys (especially those with aluminum and vanadium) combine the advantages of high strength and lightweight and are therefore used widely in the aerospace industry for the bodies and engines of airplanes (Figure 2.4). The major natural source for titanium is the ore rutile, which contains titanium dioxide (TiO2).(a) An intermediate in the preparation of elemental titanium from TiO2 is avolatile chloride of titanium (boiling point 136°C) that contains 25.24%titanium by mass. Determine the empirical formula of this compound.(b) At 136°C and atmospheric pressure, the density of this gaseous chloride is 5.6 g L-1 . Under the same conditions, the density of gaseous nitrogen (N2, molar mass 28.0 g mol-1 ) is 0.83 g L-1 . Determine the molecular formula of this compound.(c) The titanium chloride dealt with in parts (a) and (b) is produced by thereaction of chlorine with a hot mixture of titanium dioxide and coke (carbon), with carbon dioxide generated as a by-product. Write a balancedchemical equation for this reaction.(d) What mass of chlorine is needed to produce 79.2 g of the titaniumchloride?(e) The titanium chloride then reacts with liquid magnesium at 900°C to givetitanium and magnesium chloride (MgCl2). Write a balanced chemicalequation for this step in the refining of titanium.(f) Suppose the reaction chamber for part (e) contains 351 g of the titaniumchloride and 63.2 g liquid magnesium. Which is the limiting reactant? Whatmaximum mass of titanium could result?(g) Isotopic analysis of the titanium from a particular ore gave the followingresults:Isotope Relative Mass Abundance (%)46Ti 45.952633 7.9347Ti 46.95176 7.2848Ti 47.947948 73.9449Ti 48.947867 5.5150Ti 49.944789 5.34Calculate the mass of a single 48Ti atom and the average mass of the titanium atoms in this ore sample
Metallic titanium and its alloys (especially those with aluminum and vanadium) combine the advantages of high strength and lightweight and are therefore used widely in the aerospace industry for the bodies and engines of airplanes (Figure 2.4). The major natural source for titanium is the ore rutile, which contains titanium dioxide (TiO2).
(a) An intermediate in the preparation of elemental titanium from TiO2 is a
volatile chloride of titanium (boiling point 136°C) that contains 25.24%
titanium by mass. Determine the empirical formula of this compound.
(b) At 136°C and atmospheric pressure, the density of this gaseous chloride is 5.6 g L-1 . Under the same conditions, the density of gaseous nitrogen (N2, molar mass 28.0 g mol-1 ) is 0.83 g L-1 . Determine the molecular formula of this compound.
(c) The titanium chloride dealt with in parts (a) and (b) is produced by the
reaction of chlorine with a hot mixture of titanium dioxide and coke (carbon), with carbon dioxide generated as a by-product. Write a balanced
chemical equation for this reaction.
(d) What mass of chlorine is needed to produce 79.2 g of the titanium
chloride?
(e) The titanium chloride then reacts with liquid magnesium at 900°C to give
titanium and magnesium chloride (MgCl2). Write a balanced chemical
equation for this step in the refining of titanium.
(f) Suppose the reaction chamber for part (e) contains 351 g of the titanium
chloride and 63.2 g liquid magnesium. Which is the limiting reactant? What
maximum mass of titanium could result?
(g) Isotopic analysis of the titanium from a particular ore gave the following
results:
Isotope Relative Mass Abundance (%)
46Ti 45.952633 7.93
47Ti 46.95176 7.28
48Ti 47.947948 73.94
49Ti 48.947867 5.51
50Ti 49.944789 5.34
Calculate the mass of a single 48Ti atom and the average mass of the titanium atoms in this ore sample
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