Chemistry Question

Question

Titanium dioxide is converted to titanium tetrachloride by reaction with chlorine gas and carbon according to the equation

TiO₂(s) + 2Cl₂(g) + 2C(s) --> TiCl₄(g) + 2CO(g)

Suppose 40.9 g of TiO₂(s) are reacted with excess Cl₂(g), and 66.8 g of TiCl₄(g) are obtained. Calculate the percentage yield of TiCl₄(g).

Answer 1

TiO₂(s) + 2Cl₂(g) + 2C(s) --> TiCl₄(g) + 2CO(g)

Since we know that Cl2 is in excess, no need to find the limiting reactant. The moles of TiO2 will predict the amount of TiCl4 that is theoretically possible.

Molar mass TiO2 = 79.87 g/mol

Molar mass TiCl4 = 189.7 g/mol

moles TiO2 present = 40.9 g x 1 mol / 79.87 g = 0.512 mols TiO2

Theoretical yield of TiCl4 = 0.512 mol TiO2 x 1 mol TiCl4 / mol TiO2 x 189.7 g /mol = 97.1 g

Percent yield = actual yield / theoretical yield (x100%)

% yield = 66.8 g / 97.1 g (x100%) = 68.8%