Ti(s)+2Cl2(s)-TiCl4(s) compute theoretical yield in moles 8 mol Ti, 8 mol Cl2

To compute the theoretical yield of TiCl4, we need to determine the limiting reactant between Ti and Cl2.

Step 1: Write and balance the chemical equation.

Ti(s) + 2Cl2(g) → TiCl4(s)

Step 2: Calculate the moles of the reactants given.

Moles of Ti = 8 mol
Moles of Cl2 = 8 mol

Step 3: Determine the moles of TiCl4 that can be produced from each reactant.

From the balanced equation, we can see that 1 mole of Ti reacts with 2 moles of Cl2 to produce 1 mole of TiCl4.

Therefore, the theoretical yield of TiCl4 from Ti is:

Moles of TiCl4 = Moles of Ti × (1 mole TiCl4 / 1 mole Ti)
= 8 mol × (1 mole TiCl4 / 1 mole Ti)
= 8 mol

And the theoretical yield of TiCl4 from Cl2 is:

Moles of TiCl4 = Moles of Cl2 × (1 mole TiCl4 / 2 moles Cl2)
= 8 mol × (1 mole TiCl4 / 2 moles Cl2)
= 4 mol

Step 4: Determine the limiting reactant.

The limiting reactant is the one that produces the lesser amount of product. In this case, the limiting reactant is Cl2 because it produces only 4 moles of TiCl4, while Ti can produce 8 moles.

Step 5: Determine the theoretical yield.

Since Cl2 is the limiting reactant, the theoretical yield of TiCl4 is 4 mol.

To compute the theoretical yield in moles for the reaction between 8 moles of Ti (titanium) and 8 moles of Cl2 (chlorine gas), we need to determine the stoichiometry of the reaction. The balanced chemical equation for this reaction is:

Ti(s) + 2Cl2(g) --> TiCl4(s)

From the balanced equation, we can see that 1 mole of titanium (Ti) reacts with 2 moles of chlorine gas (Cl2) to produce 1 mole of titanium tetrachloride (TiCl4).

Given that we have 8 moles of Ti and 8 moles of Cl2, we need to determine the limiting reactant. The limiting reactant is the reactant that is completely consumed during the reaction. To determine the limiting reactant, we need to compare the stoichiometric ratio of the reactants.

Since 1 mole of Ti requires 2 moles of Cl2, we would need 16 moles of Cl2 to react with 8 moles of Ti (2 moles of Cl2 for each mole of Ti). However, we only have 8 moles of Cl2, which is half of what is required. Therefore, Ti is the limiting reactant in this case.

The molar ratio between Ti and TiCl4 is 1:1. Therefore, the theoretical yield of TiCl4 would be equal to the number of moles of titanium (Ti) used.

Hence, the theoretical yield of TiCl4 in moles would be 8 moles.

This is a limiting reagent problem since amounts for BOTH reactants are given. I solve these by using the first reagent, ignoring the second, and calculating the moles of the product. Then I use the second reagent, ignore the first, and calculate the moles of the product. Both answers for the product can't be correct, of course; the correct answer in limiting regent problems is ALWAYS the smaller value. Here is a worked example for soving stoichiometry problems.

http://www.jiskha.com/science/chemistry/stoichiometry.html