What is the maximum mass of TiCl4 that can be obtained from 79.0 g TiO2, 37.9 g Cl2 and excess carbon? Please show all your steps.

3 TiO2(s) + 6 Cl2 + 4 C(s) --> 3 TiCl4(g) + 2 CO2(g) + 2 CO(g)

Molar Masses:TiO2-79.88, Cl2-70.90, TiCl4-189.68

Whoa, that's a chemistry question! Looks like you're in for some chemical calculations. But don't worry, I'm here to help and entertain you along the way. Let's break it down step by step:

1. Start by calculating the moles of each compound using their molar masses:
Moles of TiO2 = 79.0 g / 79.88 g/mol
Moles of Cl2 = 37.9 g / 70.90 g/mol

2. Determine the limiting reagent. Since the balanced equation shows a 3:6 ratio between TiO2 and Cl2, let's compare the moles:
Moles of TiO2 = (79.0 g / 79.88 g/mol) = 0.988 mol
Moles of Cl2 = (37.9 g / 70.90 g/mol) = 0.534 mol

Since we need twice as many moles of Cl2, it is the limiting reagent. Sorry, TiO2, not today!

3. Now, let's use the limiting reagent to find the maximum moles of TiCl4 formed. Refer to the balanced equation:
6 moles of Cl2 reacts with 3 moles of TiCl4.

Moles of TiCl4 produced = (0.534 mol Cl2) x (3 mol TiCl4 / 6 mol Cl2)

4. Finally, convert the moles of TiCl4 to grams using its molar mass:
Mass of TiCl4 produced = (Moles of TiCl4 produced) x (189.68 g/mol)

And there you have it! You can plug in the numbers and calculate the maximum mass of TiCl4 that can be obtained. Just remember, chemistry is full of surprises, so stay on your toes!

To find the maximum mass of TiCl4 that can be obtained, we need to determine the limiting reactant. The limiting reactant is the reactant that is completely used up, limiting the amount of product that can be formed.

Step 1: Convert the given masses to moles using the molar mass.

Moles of TiO2 = mass of TiO2 / molar mass of TiO2
Moles of TiO2 = 79.0 g / 79.88 g/mol
Moles of TiO2 = 0.988 mol

Moles of Cl2 = mass of Cl2 / molar mass of Cl2
Moles of Cl2 = 37.9 g / 70.90 g/mol
Moles of Cl2 = 0.535 mol

Step 2: Use the balanced equation to determine the stoichiometric ratio between TiO2 and TiCl4.

From the balanced equation: 3 TiO2 : 3 TiCl4
So, 1 TiO2 : 1 TiCl4

Therefore, the moles of TiO2 will be equal to the moles of TiCl4 that can be obtained.

Step 3: Convert the moles of TiCl4 to mass using the molar mass.

Mass of TiCl4 = moles of TiCl4 * molar mass of TiCl4
Mass of TiCl4 = 0.988 mol * 189.68 g/mol
Mass of TiCl4 = 187.05 g

Therefore, the maximum mass of TiCl4 that can be obtained is 187.05 g.

To find the maximum mass of TiCl4 that can be obtained, we need to determine the limiting reactant in the given chemical equation. The limiting reactant is the reactant that is completely used up in the reaction, thereby limiting the amount of product that can be formed.

1. Convert the given masses of reactants into moles using the molar masses:
- Moles of TiO2: 79.0 g / 79.88 g/mol = 0.988 mol
- Moles of Cl2: 37.9 g / 70.90 g/mol = 0.534 mol

2. Use the stoichiometry of the balanced equation to determine the mole ratio between TiO2 and Cl2:
- According to the balanced equation, 3 moles of TiO2 react with 6 moles of Cl2. Therefore, the mole ratio is 3:6 or 1:2.

3. Determine the limiting reactant:
- Since the mole ratio between TiO2 and Cl2 is 1:2, for every mole of TiO2, we need 2 moles of Cl2 to react completely. However, we have only 0.534 mol of Cl2 available, which is less than the required amount. Therefore, Cl2 is the limiting reactant.

4. Calculate the maximum moles of TiCl4 that can be formed:
- Since the mole ratio between Cl2 and TiCl4 is 6:3 or 2:1, for every 2 moles of Cl2, we obtain 1 mole of TiCl4.
- Therefore, the maximum moles of TiCl4 that can be formed is equal to half the moles of Cl2, which is 0.534 mol / 2 = 0.267 mol.

5. Convert the maximum moles of TiCl4 into mass using the molar mass:
- Mass of TiCl4 = 0.267 mol × 189.68 g/mol = 50.63 g

So, the maximum mass of TiCl4 that can be obtained from the given reactants is 50.63 grams.

This is a limiting reagent (LR) problem.

1. Write and balance the equation. You have that.
2a. mols TiO2 = grams/molar mass = ?
2b. mols Cl2 = grams/molar mass = ?

3a. Using the coefficients in the balanced equation, convert mols TiO2 to mols of the product.
3b. Do the same for mols Cl2 to mols TiCl4.
3c. It is likely these two values in 3a and 3b will not agree.
3d. The correct value in LR problems is ALWAYS the smaller number and the reagent producing that number is the LR.

4. Using the smaller value, convert mols to grams. g = mols x molar mass