A 2.6g taster of Ti metal chem. combines w/ Cl gas to form 10.31g of titanium chloride?

A) What is the empircal formula? (I got TiCl4 but I'm not sure)

B) What is the percent by mass of titanium chlorine in the preview?
Answers:
A) TiCl4; you are correct

2.6 g of Ti = 0.054 moles (2.6 / 47.9)
Mass of Cl must be 10.31 g TiClx - 2.6 g Ti = 7.71
7.71 g of Cl = 0.217 moles of Cl atoms

Ti = 0.054 mol
Cl = 0.217 mol
divide both by the smallest
Ti = 1
Cl = 4

empirical formula = TiCl4

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