AP chem

A 1.25-g sample contains some of the very reactive compound Al(C6H5)3. On treating the compound with aqueous HCl, 0.951 g of C6H6 is obtained.
Al(C6H5)3(s) + 3HCl(aq) --> AlCl3(aq) + 3C6H6(l)
Assuming that Al(C6H5)3 was converted completely to products, what is the weight percent of Al(C6H5)3 in original 1.25-g sample?

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  1. This is a stoichiometry problem. Convert, using the coefficients in the balanced equation, 0.951 g C6H6 product to grams Al(C6H5)3. Then %Al(C6H5)3 = [g Al(C6H5)3/1.25)]*100 = ?

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  2. Is it 84.8%?

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  3. I got 83.8%. close enough. just make sure not to round your values until the very end (keep them in your calc).

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  4. I don't understand how you got to 83.8%??

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