In the following reaction, how many grams of ferrous sulfide (FeS) will produce 0.56 grams of iron (III) oxide (Fe2O3)?
4FeS + 7O2 d 2Fe2O3 + 4SO2

The molar mass of ferrous sulfide is 87.92 grams and that of iron (III) oxide is 159.7 grams.

Question

In the following reaction, how many grams of ferrous sulfide (FeS) will produce 0.56 grams of iron (III) oxide (Fe2O3)?
4FeS + 7O2 d 2Fe2O3 + 4SO2

The molar mass of ferrous sulfide is 87.92 grams and that of iron (III) oxide is 159.7 grams.

ilovebmth1234 · Answer

A. 0.1541 grams
B. 0.6166 grams
C. 0.5085 grams
D. 2.0344 grams

ilovebmth1234 · Answer

@Jack_Prism

rushwr · Answer

Show me ur work and ur answer !

ilovebmth1234 · Answer

@magicremix123

rushwr · Answer

look at the mole ratio between Fe2O3 and FeS that is 2:4 right?
We can find the no of moles of Fe2O3
moles= mass divided by molar mass
Moles of Fe2)3 = o.56g/ 159.7= 0.003506moles
As we can see FeS has twice the moles as Fe2O3 so moles of FeS = 0.00351*2 = 0.007013
Moles = mass/molar mass
mass= moles*molar mass
mass of FeS = 0.007013 * 87.92= 0.6166g So the answer is B

anonymous · Answer

I would say c.) Thats what i got .....mhm

anonymous · Answer

Maybe, i did something wrong in the problem