What is percent yield of this reaction?

The following reaction occurred in lab. The student obtained 425g of titatnium (IV) chloride from 4.15 mol TiO2, 5.67 mol C and 6.78 mol Cl2. What is the percent yield of this reaction!

Im studying for an exam, so if you could explain the steps I would really appreciate it :)

Thanks in advance!

1 Answer
Nov 30, 2017

Step 1: Balance the chemical reaction.

TiO_2+2C+2Cl_2->TiCl_4+2CO

Step 2: Find the limiting reagent.

The limiting reagent in this reaction will be C because for every 1 mole of TiO_2 you need 2 moles of C and Cl_2. We don't have twice the number of moles of TiO_2 for C or Cl_2, so not all of the TiO_2 will react.

Thus, we resort to the compound we have the least of next since we need the same number of moles of C and Cl_2 (twice the moles of TiO_2), which will be C.

Step 3: Find the theoretical yield of TiCl_4 by performing the steps below.

Step 4: Use the mole ratio between C and TiCl_4 to find how many moles of TiCl_4 will be produced.

"5.67 moles C"*(("1 mole" TiCl_4)/("2 moles C"))= "2.84 moles" TiCl_4

Step 4: Convert moles of TiCl_4 to grams using its molar mass to find the theoretical yield.

"2.84 moles" TiCl_4*(("189.679 grams")/("1 mole" TiCl_4))= "539 grams" TiCl_4

Step 5: Use the theoretical yield and the actual yield to calculate the percent yield using the equation:

"%yield"=("actual yield"/"theoretical yield")*100

Thus, we can plug in:

"%yield"=("425 grams"/"539 grams")*100=78.8

Finally, our percent yield is 78.8%.

I hope this helps for your exam!