Question

When TiCl4 (s) reacts with H20 (l), the products TiO2 (s) and HCl (g) are formed. If there is 87.3 g of
titanium (IV) chloride present, with water in excess, how much solid titanium (IV) oxide (in grams)
could theoretically be produced?

Answer 1

The mass of titanium (IV) oxide produced is 36.7 grams.

Given:

The reaction between titanium (IV) chloride and water.

$TiCl_4(s)+2H_2O(l)\rightarrow TiO_2(s)+4HCl(g)$

The mass of titanium (IV) chloride is 87.3 g.

To find:

The mass of titanium (IV) oxide produced.

Solution:

The mass of titanium (IV) chloride = 87.3 g.

Moles of titanium (IV) chloride =$\frac{87.3 g}{189.679 g/mol}=0.460 mol$

$TiCl_4(s)+2H_2O(l)\rightarrow TiO_2(s)+4HCl(g)$

According to reaction, 1 mole of titanium (IV) chloride gives 1 mole of titanium (IV) oxide, then 0.460 moles of titanium (IV) chloride will give:

$=\frac{1}{1}\times 0.460 mol=0.460\text{ mol of }TiO_2$

Mass of 0.460 moles of  titanium (IV) oxide:

$= 0.460mol\times 79.866 g/mol =36.7 g$

The mass of titanium (IV) oxide produced is 36.7 grams.

Learn more about the unitary method here:

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