What mass of TiCl4 must react with an excess of water to produce 50.0g of TiO2 if the reaction has a 78.9% yield

\large \boxed{\text{150 g TiCl}_{4}}  

Explanation:

We will need a balanced chemical equation with masses and molar masses, so, let's gather all the information in one place.

Mᵣ:     189.68                  79.87

           TiCl₄ + 2H₂O ⟶ TiO₂ + 4HCl

m/g:                                 50.0

To solve this stoichiometry problem, you must

Convert the actual yield to the theoretical yield  Use the molar mass of TiO₂ to convert the theoretical yield of TiO₂ to moles of TiO₂ Use the molar ratio to convert moles of TiO₂ to moles of TiCl₄ Use the molar mass of TiCl₄ to convert moles of TiCl₄ to mass of TiCt₄

1. Theoretical yield of TiO₂

2.  Moles of TiO₂

3,  Moles of TiCl₄

The molar ratio is 1 mol TiO₂:1 mol TiCl₄.

4.  Mass of TiCl₄

Hydrogen is the most abundant element on the periodic table..hope it .

What are the options? i can you if you give them.