My Math Forum Limiting Reactants and Percent Yield

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 February 26th, 2011, 06:59 PM #1 Member   Joined: Feb 2011 Posts: 49 Thanks: 0 Limiting Reactants and Percent Yield Aluminum burns in bromine, producing aluminum bromide: 2Al (s) + 3 Br subcipt 2 (l) ---> 2AlBr subcript 3 (s) In a certain experiment, 6.0 g aluminum was reacted with an excess of bromine to yield 50.3 g aluminum bromide. Calculate the theoretical and percent yields for this experiment. Can you please help with the steps for this problem?
 March 12th, 2011, 07:23 PM #2 Senior Member   Joined: Nov 2006 From: I'm a figment of my own imagination :? Posts: 848 Thanks: 0 Re: Limiting Reactants and Percent Yield All problems of this form follow the same general procedure. You're given the mass of one of the reactants present, and you want to convert that to a number of moles. From there you can determine the number of moles of the product that should be present after the reaction and then convert that back to a mass. This is the theoretical yeild. Then the percent yield is simply the given mass of product divided by the theoretical yeild and expressed as a percentage. Did that answer your question?

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# aluminum burns in bromine

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