perhaps some information might help.
it seems, after reading the packet a couple times, the main equation to be used in order to determine is going to be:
n(H2) = (0.0556 moles H2 / gAl) * X*gAl + (0.0153 moles H2 / gZn) * (mass of sample - X)
where X is apparently the mass of Aluminum, (mass of Al -X) is the mass of Zinc
that is that for the equation they give that I still have to try and make some sense about.
as for the value that I have acquired through the experimentation, at least the values that are significant:
mass of alloy = .104 g
displaced water = 122.5 mL (we are to assume density of the water is 1.00 g/mL to determine the the amount of hydrogen gas available)
the temperature was 22 Celsius (of the water that is)
barometric pressure = 761.4 mm Hg
pressure of water = 19.87 mm Hg
pressure of hydrogen = 741.6 mm Hg
and I am supposed to determine the mass of Al, Zn the percentage of Al and Zn.
I am not asking for you to do the work, but to tell me how this works, I am completely lost...
(P.S. use ideal gas laws... do not get too technical, this is a beginners chemistry course, sort of)
if you feel like giving the response rather than explaining that will also help, I could use a response to try and work it backwards, answers by themselves are pretty useless for me though as I have to also write a lab report explaining everything.