About half the world's production of pigments for paints involves the formation of white TiO2. It is made on a large scale by the chloride process , starting with ores containing only small amounts of rutile, TiO2. The ore is treated with chlorine and carbon. this produces TiCl4 and gaeseous product according to the following equation:
3TiO2(s)+ 4C(s)+ 6Cl2(g)--> 3TiCl4(l)+ 2CO2(g)+ 2CO(g)
the titanium(IV)chloride is then converted into titanium(IV)oxide of high purity
TiCl4(l)+ O2(g)--> TiO2(s)+ 2Cl2(g)
suppose the first process can be carried out with 70.0% yield and then second one with 93.0% yield. How many kilograms of TiO2 could be produced starting with 1.00metric ton (1.00x10^6g)of an ore that is 0.75% rutile TiO2?
College Chemistry - DrBob222, Sunday, October 16, 2011 at 9:25pm
Here is a worked example of a stoichiometry problem Your problem has two such problems in it (or you can combine the two if you wish).
Convert 1 metric ton to grams ore then to grams TiO2 (using the 0.75% in the ore), then to g TiCl4 (using the 70%%) and finally to TiO2 final product (using the 93.0%). Post your work if you get stuck.
College Chemistry - Anonymous, Monday, October 17, 2011 at 12:11am
i converted the 1metric ton to grams but then how to i convert it to grams of TiO2(using the 0.75% in the ore)