Consider the following chemical equation:

TiCl4(g) + 2Mg(l) → Ti(s) + 2MgCl2(l)
3.54×107g of TiCl4(g) were reacted completely and 7.91×106g of Ti(s) was obtained in the experiment.

a. Calculate the theoretical yield of Ti(s).

b.What is the actual yield of Ti(s) in this experiment?

c.Calculate the % yield of Ti(s) in this experiment.

Remember how to work this type stoichiometry problem.

Step 1. Convert what you have (in this case TiCl4) to mols. mols = grams/molar mass

Step 2. Using the coefficients in the balanced equation, convert mols of what you have to mols of what you want(in this case Ti). With the coefficients you can convert anything to anything.
mols TiCl4 x (1 mol Ti/1 mol TiCl4) = mols TiCl4 x 1/1 = ?

Step 3. Now convert mols of what you have to grams. grams = mols Ti x atomic mass Ti. This is the theoretical yield (i.e., as if it were 100%). Let's call this TY for theoretical yield.

Step 4. It isn't 100%. The actual yield from the problem is 7.91E6 g. Let's call this AY for actual yield.

Step 5. % yield = (AY/TY)*100 = ?

Print this out. This five step procedure will work all of the stoichiometry problems (limiting reagent problems take an extra step) and if the problem is solution mols = M x L.

Thanks DrBob222!!! You have helped me so much!!

To calculate the theoretical yield of Ti(s), we need to determine the stoichiometry of the reaction. From the balanced chemical equation, we can see that 1 mole of TiCl4 reacts with 2 moles of Mg to produce 1 mole of Ti.

a. Calculate the theoretical yield of Ti(s):
1. Determine the moles of TiCl4 used:
- The molar mass of TiCl4 is 189.68 g/mol (the sum of the atomic masses of titanium and chlorine).
- Divide the given mass of TiCl4 (3.54×10^7 g) by its molar mass to get the moles:
moles of TiCl4 = (3.54×10^7 g) / (189.68 g/mol)

2. Determine the moles of Ti obtained using stoichiometry:
- According to the stoichiometry, for every 1 mole of TiCl4, we obtain 1 mole of Ti.
- Therefore, the moles of Ti obtained is equal to the moles of TiCl4 used.

3. Calculate the theoretical yield of Ti(s) in grams:
- Multiply the moles of Ti obtained by the molar mass of Ti, which is 47.867 g/mol (atomic mass of titanium):
theoretical yield of Ti(s) = moles of Ti × molar mass of Ti

b. To find the actual yield of Ti(s), we use the given mass of Ti(s) obtained in the experiment, which is 7.91×10^6g.

c. Calculate the % yield of Ti(s) in this experiment:
- Divide the actual yield of Ti(s) by the theoretical yield of Ti(s) and multiply by 100 to obtain the percentage:
% yield = (actual yield / theoretical yield) × 100

Now you can substitute the values mentioned in the question into the formulas to find the answers.