Posted by ana on Sunday, September 9, 2007 at 8:00pm.
You need to determine the percent composition of Zn in ZnCl2 based on atomic masses and the formula. Then, you can get the grams of Zn recovered.
This doesn't change Bob Pursley's answer but let me try to help so you will "get the question." The idea in any analytical scheme is to start with a known mass of substance and convert it to something else that is known. You started with brass and converted the Zn in the brass to ZnCl2. Then the ZnCl2 was weighed. Grams ZnCl2 can be converted to mols Zn and to grams Zn and (g Zn/g sample)*100 = %Zn. The idea is to work backwards from what you can weigh to determine how much of a material you MUST have started with. For the second part, think about this as a hint:
What else is produced in addition to the ZnCl2 and how might you use that to determine the amount of Zn in the brass alloy?
I'm sorry to be such a big bother but I just want to make sure I did it the right way.
(.0985gZnCl2)(1molZnCl2)/(136.28gZnCl2)
I got(7.23times10withthe exponent-4 mols)
Then I converted moles of ZnCl2 to mol of Zn using themole to mole ratio. Then I converted moles of Zn to grams, and then I didvided the mass of Zn by the mass of ZnCl and times it by a hundred. And I got .03468 (which I think is a very small number), then I multiply the mass in the reactant side .5065g by the percentage which was (3.4times10exponent-4) (igot this by dividing .03468 by 100).
My final answer was (1.7568times10 exponent-4) I will really appreciate If you tell If I'm right, I'm a little unconfident in regard to the answer because is such a small number. Thank you again in advance. Also thank you very much both bobpursleyand Drbob222, your answers where as you might already know very helpfull.
use stoich to convert into grams of Zn then find percentage like normal
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