If you begin with 14.0g of TiCl4(1), how many liters of H2O(g) will need?

3.32 L

Explanation:

Step 1: Write the balanced equation

TiCl₄(l) + 2 H₂O(g) → TiO₂(s) + 4 HCl(g)

Step 2: Calculate the moles corresponding to 14.0 g of TiCl₄

The molar mass of TiCl₄ is 189.68 g/mol.

14.0 g × 1 mol/189.68 g = 0.0738 mol

Step 3: Calculate the moles of H₂O needed to react with 0.0738 moles of TiCl₄

The molar ratio of TiCl₄ to H₂O is 1:2. The moles of H₂O needed are 2/1 × 0.0738 mol = 0.148 mol

Step 4: Calculate the volume corresponding to 0.148 moles of H₂O(g)

At standard temperature and pressure, 1 mole of H₂O(g) has a volume of 22.4 L.

0.148 mol × 22.4 L/1 mol = 3.32 L

the correct answer is option d

explanation:

i was wrong its d because they dont use cm when calculating square roots

c8h10 is your answerr