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How many grams of #TiCl_4# are needed to produce 44.9 g of titanium?

Answer 1

Avery Adams

At least #178*g# of #"titanic chloride"# are required...........

#"Moles of titanium"# #=# #(44.9*g)/(47.87*g*mol^-1)=0.938*mol.#

And thus we need AT LEAST an equimolar quantity of #TiCl_4#.

Additionally, this is an equivalent mass of:

#0.938*molxx189.68*g*mol^-1=??*g.#

I think the industrial process utilizes either alkali metals or alkaline earth metals to reduce the #TiCl_4#.

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Answer 2

Mateo Aguilar

The molar ratio of TiCl4 to titanium is 189.68 g/mol, and the molar mass of titanium is 47.87 g/mol. Based on this molar ratio, we can create a proportion to determine the quantity of TiCl4 required: [ \frac{44.9 \text{ g Ti}}{1} \times \frac{1 \text{ mol TiCl}_4}{47.87 \text{ g Ti}} \times \frac{189.68 \text{ g TiCl}_4}{1 \text{ mol TiCl}_4} = \text{mass of TiCl}_4 ]

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Answer from HIX Tutor

When evaluating a one-sided limit, you need to be careful when a quantity is approaching zero since its sign is different depending on which way it is approaching zero from. Let us look at some examples.