Question

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!

Answer 1

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!