🤓 Based on our data, we think this question is relevant for Professor Lampropoulos's class at UNF.

Reactants:

titanium metal → Ti

chlorine gas → Cl_{2}

Products:

titanium (IV) chloride → TiCl_{4}

**Balanced reaction: Ti + 2 Cl _{2} → TiCl_{4}**

**Calculate theoretical yield:**

**TiCl**_{4}** from ****Ti:**

molar mass TiCl_{4} = 189.667 g/mol

molar mass Ti = 47.867 g/mol

$\mathbf{mass}\mathbf{}{\mathbf{TiCl}}_{\mathbf{4}}\mathbf{=}\mathbf{3}\mathbf{.}\mathbf{00}\mathbf{}\overline{)\mathbf{g}\mathbf{}\mathbf{Ti}}\mathbf{\times}\frac{\mathbf{1}\mathbf{}\overline{)\mathbf{mol}\mathbf{}\mathbf{Ti}}}{\mathbf{47}\mathbf{.}\mathbf{867}\mathbf{}\overline{)\mathbf{g}\mathbf{}\mathbf{Ti}}}\mathbf{\times}\frac{\mathbf{1}\mathbf{}\overline{)\mathbf{mol}\mathbf{}{\mathbf{TiCl}}_{\mathbf{4}}}}{\mathbf{1}\mathbf{}\overline{)\mathbf{mol}\mathbf{}\mathbf{Ti}}}\mathbf{\times}\frac{\mathbf{189}\mathbf{.}\mathbf{667}\mathbf{}\mathbf{g}\mathbf{}{\mathbf{TiCl}}_{\mathbf{4}}}{\overline{)\mathbf{1}\mathbf{}\mathbf{mol}\mathbf{}{\mathbf{TiCl}}_{\mathbf{4}}}}$

If 3.00 g of titanium metal is reacted with 6.00 g of chlorine gas, Cl_{2}, to form 7.7 g of titanium (IV) chloride in a combination reaction, what is the percent yield of the product?

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Based on our data, we think this problem is relevant for Professor Lampropoulos's class at UNF.