Just follow the steps in this example.
http://www.jiskha.com/science/chemistry/stoichiometry.html
If you have Hydrochloric acid, how many grams of aluminum must you use to produce 57.0 L of hydrogen at STP?
2Al(s)+6HCl(aq) --> 3H2(g)+2AlCl3(aq)
4 answers
I ended up getting 42.718333 not rounded to sig figs but does the excess of hydrochloric acid have anything to do with the answer and what about the STP?
I have something like 45. something and the problem says nothing about excess HCl; however, it won't work this way unless HCl IS IN excess.
You use the 57.0 L at STP to calculate moles H2. Remember that 1 mole of a gas at STP occupies 22.4 L; therefore, 57.0/22.4 = ?? moles H2.
Then ?? moles H2 x (2 moles Al/3 moles H2) = ?? moles H2 x (2/3) = moles Al and that times molar mass Al = about 45 g or so Al.
You use the 57.0 L at STP to calculate moles H2. Remember that 1 mole of a gas at STP occupies 22.4 L; therefore, 57.0/22.4 = ?? moles H2.
Then ?? moles H2 x (2 moles Al/3 moles H2) = ?? moles H2 x (2/3) = moles Al and that times molar mass Al = about 45 g or so Al.
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1 answer