Question

Titanium, which is used to make airplane engines and frames can be obtained from titanium tetrachloride, which in turn is obtained from titanium oxide by the following process:

$3Ti{O}_2\left(s\right)+4C\left(s\right)+6{Cl}_2\left(g\right)⟶{3TiCl}_4\left(g\right)+2{CO}_2\left(g\right)+2CO\left(g\right)$

A vessel contains $4.32$ g ${TiO}_2$, $5.76$ g $C$ and $7.1$ g ${Cl}_2$. Suppose the reaction goes to completion as written, how many grams of ${TiCl}_4$ can be produced?

• A. $9.8$ g
• B. $9.5$ g
• C. $8.1$ g
• D. $8.5$ g

Answer 1

The correct option is B $9.5$ g

The balanced reaction is given below:
$3Ti{O}_2+4C+6C{l}_2\to 3TiC{l}_4+2C{O}_2+2CO$

Mass given: $4.32$ g $5.76$ g $7.1$ g

No. of moles: $\frac{4.32}{80}$ $\frac{5.76}{12}$ $\frac{7.1}{71}$

=$0.054$ =$0.48$ =$0.1$

Ratio of moles given
and stoichiometry $\frac{0.054}{3}$ $\frac{0.48}{4}$ $\frac{0.1}{6}$

coefficient: =$0.018$ =$0.12$ =$0.017$

As $0.017$ is lowest, $C{l}_2$ is limiting reagent and product will form according to number of moles of $C{l}_2$.

So, moles produced of $TiC{l}_4=\frac{3}{6}\times 0.1=0.05$ moles.

And mass produced of $TiC{l}_4=0.05\times 190=9.5$ g.