Asked by Hannah

5. How many grams of iron oxide can be produced from 2.50 g of oxygen reacting with iron, according to the following equation?
2 Fe (s) + 3 O2 (g) -->2 Fe2O3(s)
Answered by Scott
answered
Answered by semisi caucau
in order to solve this problem, the best way is to calculate their mole ratio(O2 and Fe2O3).so that would be
mole ratio of O2 and Fe2O3;it would be 3:2=2.50g:x..3X=5 so the mole for fe2o3 is 1.67mol....so u got the mole so find the the mass...formula is moles=mass/Mr(Fe2O3)....1.67mol=mass/272g/mol..thus ur answr comes to 454.24g...therefore the mass o iron oxide comes to 454.24grams..
Answered by DrBob222
No that's not right.
mols O2 = 2.50g/32 = 0.078 but you should do it more accurately.
Convert to mols Fe2O3. That's 0.078 x 2/3 = approx 0.052
Then g Fe2O3 = mols x molar mass = 0.052 x 159.7 = approx 8.3.
Answered by TONY
Calculate the mass of iron needed to completely react with oxygen to produce 5.50 g iron
(TI) oxide.
A Fe + 302
› 2 Fe203
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