Question

1. Titanium tetrachloride, Ticle will react with titanium to produce titaniun trichloride TiCl + Ti → Tich (unbalanced) First balance the equation, then answer: If 4.00 g of TiCliis mixed with 6.00 g of Ti.... w how many grims of Tich is produced? b) Which starting material is in excess, and how many What is the percent yield if 3.45 g of Tich is actually collected?

Answer 1

Balanced equation: 3 TiCl4 + Ti $\rightarrow$ 4 TiCl3

a) Moles of Ti = mass / molar mass = 6 / 47.9 = 0.125 moles

moles of TiCl4 = mass / molar mass = 4 / 189.7 = 0.0211 moles

From the equation, moles of TiCl4 needed = 3 * moles of Ti = 3 * 0.125 = 0.375 moles

This is more than the amount availbale making TiCl4 the limiting reagent.

Moles of tiCl3 = Moles of TiCl4 * 4 / 3 = 0.0211 * 4/3 = 0.0281 moles

Mass of TiCl3 = moles * molar mass = 0.0281 * 154.2 = 4.333 g

b) We know that Ti is in excess. Moles of Ti reacted = Moles of TiCl4 / 3 = 0.0211 / 3 = 0.007

Moles of Ti left = initial - reacted = 0.125 - 0.007 = 0.118 moles

Mass remaining = moles * molar mass = 0.118 * 47.9 = 5.652 g

c) theoretical yield = 4.333 g

% yirld = actual mass / theoretical mass * 100 = 3.45 / 4.333 *100 = 79.68%