Question

What is the maximum mass of `"TiCl"_4` that can be obtained from 60.5 g `"TiO"_2`, 59.9 g `"Cl"_2` and excess carbon?

Give your answer in grams to three significant figures.

The balanced chemical equation for the reaction is given below.

`3"TiO"_2(s)+6"Cl"_2+4"C"(s)->3"TiCl"_4(g)+2"CO"_2(g)+2"CO"(g)`

Answer 1

`80.2g`

Explanation:

With excess carbon we only need to determine whether the amount of chlorine is limiting or not. Then we calculate the produce `TiCl_4` from the known moles of chlorine.
We need two moles of `Cl_2` for every `Ti` atom.
`59.9/70.9 = 0.845` moles `Cl_2`
(we could also do the calculation precisely using a Cl atom and 35.45g/mol, but we already know it is doubled in this reaction).

`60.5/47.87 = 1.264` moles of Ti. Therefore, `Cl_2` is limiting.

We can ONLY produce `0.845/2 = 0.423` moles of `TiCl_4` formed from the same number of moles of `TiO_2`.

The mass is `0.423mol xx 189.67(g/(mol)) = 80.23g` or just `80.2g` for three significant figures.