[Angel_luvusa]

Hey you guys,

I really hate to post a homework problem on soompi >.< But I've gotten extremely desperate because this is my last chance at an A in the class. So if anybody could help me, I'd be forever grateful. The problem is:

In 1897 the Swedish explorer Andree tried to reach the North Pole in a balloon. The balloon was filled with hydrogen gas. The hydrogen gas was prepared from iron splints and sulfuric acid. The reaction is:

H2SO4(aq) + Fe(s) → FeSO4 + H2(g)

The volume of the balloon was 5800 m3 and the loss of hydrogen gas during filling was estimated at 17.0%. What mass of iron splints and H2SO4(aq) were needed to ensure that complete filling of the balloon? Assume a temperature at -2.3 °C, a pressure of 747 torr, and 100% yield.

I believe that I'll use the gas law M= (dRT)/(P) ?

I first converted the volume to liters (since the rate uses liters) and got 5.8*10^6.. and then I found the density (83g H)/(5.8*10^6)= 1.4*10^-5 g/L

The equation i had then set up was M= (1.4*10^-5g/l)(0.08206 (l*atm/m-k))(270.7K)/ (.98 atm)

I then get that the molar weight of Hydrogen is 3.17*10^-4

From there I just used the equation and the weight of hydrogen to do stocheometry to get the weights for Fe and H2SO4. I'm pretty sure i'm doing it wrong though.. Once again, thanks for taking the time to read this and I appreciate anyone's help. =]

[Aeroshark2000]

see below

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[f0reveralways]

uh.

1.73 x 10^7 grams of Fe
and 3.03 x 10 ^7 grams of H2SO4

.. i think? lol.

Anyway,
Google is your best friend

[Angel_luvusa]

Thank you both so much. =] I really appreciate it.