What mass of TiCl4 must react with an excess of water to produce 50.0 g of TiO2 if the reaction has a 78.9% yield? #TiCl_4 + 2H_2O → TiO_2 + 4HCl#

1 Answer
anor277
Jun 24, 2018

We address the equation...

#TiCl_4(l) + 2H_2O(l) rarr TiO_2(s) + 4HCl(aq)#

I gets approx. #150*g#...

Explanation:

We gots a #50*g# mass of #"titanic oxide..."#

#"Moles of titanic oxide"-=(50*g)/(79.87*g*mol^-1)=0.626*mol#

But this was produced in a #78.9%# yield....and so we take a mass of #"titanic chloride"# of...

#(0.626*molxx189.68*g*mol^-1)/(0.789)=??*g#

Incidentally, do you know the main application of titanic oxide? Vast quantities are used in the paints and pigments industry to produce #"the white that is whiter than white..."#

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