Asked by Yoni
If 10.0 L of hydrogen collected over water at 20' C and 750 mm Hg are produced, how many grams of iron metal must react with excess steam?
Answers
Answered by
DrBob222
Do you have a reaction equation? One source gives Fe2O3 as the product; another gives Fe3O4 as the product. The answer to this question depends upon which product is formed. I will assume Fe2O3 and go from there.
2Fe + 3H2O ==> Fe2O3 + 3H2
Use PV = nRT and solve for n = mols H2 at the conditions listed.Remember T must be in kelvin and P in atmospheres (750 mm/760mm = ? atm)
Then convert mols H2 to mols Fe.
mols Fe needed = mols H2 x (2 mols Fe/3 mols H2) = mols H2 x 2/3 = ?
Finally, convert mols Fe to grams. g Fe = mols Fe x atomic mass Fe = ?
2Fe + 3H2O ==> Fe2O3 + 3H2
Use PV = nRT and solve for n = mols H2 at the conditions listed.Remember T must be in kelvin and P in atmospheres (750 mm/760mm = ? atm)
Then convert mols H2 to mols Fe.
mols Fe needed = mols H2 x (2 mols Fe/3 mols H2) = mols H2 x 2/3 = ?
Finally, convert mols Fe to grams. g Fe = mols Fe x atomic mass Fe = ?
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