Question

Titanium tetrachloride (TiCl$_4$) reacts with THF to form an octahedral complex X under inert atmosphere at 25°C. If 5.0 g of TiCl$_4$ is used and the yield is 80%, the amount of X (in grams) formed is .......... (Round off to one decimal place) (Use atomic weights: Ti = 48, Cl = 35.5, O = 16, C = 12, H = 1)

Hint:

Always account for yield in reactions, as the actual amount of product will be less than the theoretical amount.

Answer 1

Correct Answer: 6.9

Step 1: Calculating Moles of TiCl$_4$.
First, we calculate the moles of TiCl$_4$ used in the reaction: \[ \text{Moles of TiCl}_4 = \frac{\text{Mass of TiCl}_4}{\text{Molar mass of TiCl}_4} \] Using the atomic masses, the molar mass of TiCl$_4$ is calculated.

Step 2: Calculating the Amount of X Formed.
Since the yield is 80%, the actual amount of X formed is 80% of the theoretical amount. Using the calculated moles of TiCl$_4$, we determine the mass of X produced.

Step 3: Conclusion.
The amount of X formed is 3.2 g.