What mass of Cl2 gas is needed to react with 2.48 mol TiO2

To produce what? What equation do you have in mind?

My best guess. 2Cl2 + TiO2 + C ==> TiCl4 + CO2

mols TiO2 = 2.48
Use the coefficients in the balanced equation to obtain
mols Cl2 = 2.48 x (2 mols Cl2/1 mol TiO2) = 2.48*2 = ?
Then grams = mols Cl2 x molar mass Cl2 = ?

To find the mass of Cl2 gas needed to react with 2.48 mol of TiO2, we need to use the balanced chemical equation for the reaction.

The balanced equation for the reaction between Cl2 and TiO2 is:

2Cl2 + 3TiO2 -> TiCl4 + 2TiO2

From the balanced equation, we can determine the stoichiometric ratio between Cl2 and TiO2. It shows that 2 moles of Cl2 react with 3 moles of TiO2.

Therefore, we can set up a proportion to find the mass of Cl2 gas:

(2 mol Cl2 / 3 mol TiO2) = (x g Cl2 / 2.48 mol TiO2)

We can solve this proportion by cross-multiplication:

2 mol Cl2 * 2.48 mol TiO2 = 3 mol TiO2 * x g Cl2

4.96 mol Cl2 = 3 mol TiO2 * x g Cl2

Divide both sides of the equation by 4.96 mol Cl2:

x g Cl2 = (3 mol TiO2 * x g Cl2) / 4.96 mol Cl2

Simplifying, we find:

x g Cl2 = 0.605 g Cl2

Therefore, approximately 0.605 grams of Cl2 gas is needed to react with 2.48 mol of TiO2.