Question

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

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Answer 1

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

Step-by-step 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

`\text{Theoretical yield} = \text{50.0 g actual} * \frac{\text{100 g theoretical}}{\text{78.9 g actual}} = \text{63.37 g theoretical}`

2. Moles of TiO₂

`\text{Mass of TiO}_(2) = \text{63.37 g TiO}_(2) * \frac{\text{1 mol TiO}_(2)}{\text{79.87 g TiO}_(2) } = \text{0.7934 mol TiO}_(2)`

3, Moles of TiCl₄

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

`\text{Moles of TiCl}_(4) = \text{0.7934 mol TiO}_(2) * \frac{\text{1 mol TiCl}_(4)}{\text{1 mol TiO}_(2)} = \text{0.7934 mol TiCl}_(4)`

4. Mass of TiCl₄

`\text{Mass of TiCl}_(4) = \text{0.7934 mol TiCl}_(4) * \frac{\text{189.98 g TiCl}_(4)}{\text{1 mol TiCl}_(4)} =\textbf{150 g TiCl}_{\mathbf{4}} \\\\\text{You must use $\large \boxed{\textbf{150 g TiCl}_{\mathbf{4}}}$}`