1. Chlorine was passed over 2.14 g of heated titanium and 6.88 g of a chloride containing compound of Ti was obtained. What is the empirical formula of the chloride containing compound?
My Work:
2.14g Ti X ( 1mol Ti / 48g Ti) = 0.14333 mol Ti
I know im suppose to find the moles of Chlorine from the compound and then get the ratios. Im having trouble finding the moles of Cl though.
The answer is suppose to be TiCl3
My Work:
2.14g Ti X ( 1mol Ti / 48g Ti) = 0.14333 mol Ti
I know im suppose to find the moles of Chlorine from the compound and then get the ratios. Im having trouble finding the moles of Cl though.
The answer is suppose to be TiCl3
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The amount of chlorine in the compound must be 6.88 - 2.14 = 4.74 g chlorine
4.74 g Cl (1 mol Cl / 35.453 g Cl) = .1337 mol Cl
But wait, 2.14 g Ti ( 1 mol Ti / 48 g Ti) =.0446 mol Ti , you had an error in your calculation (or maybe just a typo)
Now divide the number of moles of Ti and of Cl by the smallest, which is .0446. You get 1 for Ti and 3 for Cl, therefore TiCl3 is the empirical formula.
4.74 g Cl (1 mol Cl / 35.453 g Cl) = .1337 mol Cl
But wait, 2.14 g Ti ( 1 mol Ti / 48 g Ti) =.0446 mol Ti , you had an error in your calculation (or maybe just a typo)
Now divide the number of moles of Ti and of Cl by the smallest, which is .0446. You get 1 for Ti and 3 for Cl, therefore TiCl3 is the empirical formula.