How much titanium is produced from 380 g of titanium chloride?

To determine how much titanium is produced from 380 g of titanium chloride (TiCl4), we need to use stoichiometry based on the chemical equation for the reduction of titanium chloride to titanium metal. Typically, titanium is produced through the Kroll process, in which titanium chloride is reduced by magnesium:

\[ TiCl_4 + 2Mg \rightarrow Ti + 2MgCl_2 \]

From the balanced chemical equation, we can see that 1 mole of titanium chloride yields 1 mole of titanium. To find out how many moles of titanium that 380 g of titanium chloride will produce, we need the molar mass of titanium chloride.

The molar mass of titanium (Ti) is approximately 47.87 g/mol, and the molar mass of chlorine (Cl) is approximately 35.45 g/mol. Since there are four chlorine atoms in titanium chloride, the molar mass of titanium chloride (TiCl4) is:

\[ \text{Molar mass of } TiCl_4 = 47.87 + (4 \times 35.45) \] \[ \text{Molar mass of } TiCl_4 = 47.87 + 141.80 \] \[ \text{Molar mass of } TiCl_4 = 189.67 \text{ g/mol} \]

Now we can find out the amount of titanium that can be produced from 380 g of titanium chloride:

\[ \text{Moles of } TiCl_4 = \frac{\text{Mass of } TiCl_4}{\text{Molar mass of } TiCl_4} \] \[ \text{Moles of } TiCl_4 = \frac{380 \text{ g}}{189.67 \text{ g/mol}} \] \[ \text{Moles of } TiCl_4 = 2 \text{ moles (approximately)} \]

Given the 1:1 molar ratio from the chemical equation, this means that 2 moles of TiCl4 will produce 2 moles of titanium.

To find the mass of this titanium, we use the molar mass of titanium:

\[ \text{Mass of Titanium} = \text{Moles of Titanium} \times \text{Molar Mass of Titanium} \] \[ \text{Mass of Titanium} = 2 \times 47.87 \text{ g/mol} \] \[ \text{Mass of Titanium} = 95.74 \text{ g (approximately)} \]

Therefore, 380 g of titanium chloride will produce approximately 95.74 g of titanium.