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)#

1 Answer
SCooke
Oct 1, 2017

#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.

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