help me solve this chem problem?

Question

Fe2O3+ CO -----> Fe+ CO2

How many grams of Fe2O3 will be required to produce 5.90 moles of Fe?

Answer 1

Since the equation you listed isn't balanced, I'm going to attempt that first:

Fe2O3 + 3(CO) ----> 2Fe + 3(CO2)

since 1 mole of Fe2O3 seems to produce 2 moles of Fe, it would appear we need 5.9/2 = 2.95 moles of Fe2O3

Given that 1 mole of these elements weighs: (see source)
O = 16g
Fe = 56g

2.95 moles * ( 2 * 56g + 3 * 16g ) = 2.95 * 160g = 472g

Hope that helps.

Answer 2

This is a simple atomic mass question. Atomic mass really means
x grams of the atom/molecule per mole. An atom of Oxygen is ~16.00 grams/mole, Carbon ~12.01 grams/mole and iron is 55.85 grams/mole. The first thing we must do is realize that the equation isnt really balanced, so we balance it.
Fe2O3 + 3CO ---->2Fe + 3CO2

So for every mole of FE2O3 we will get 2 moles of Fe, so to get 5.90 moles of Fe, we need 2.95 moles of Fe2O3. Then we simply find the atomic weight of Fe2O3:

2*55.85+3*16=159.7 grams of Fe2O3 / mole

Multiply that by the number of moles we want (2.90)
463.13 grams of Fe2O3

Answer 3

balanced eq: Fe2O3 + CO --> 2Fe+ CO2
grams of Fe2O3? to produce 5.9 moles of Fe
u need a periodic table to find their molecular mass:

Fe2O3= (2x55.85 + 3 x 16)= 159.7 g

use stoichiometry
(x in moles Fe2O3)( 2 moles of Fe / 1 mole of Fe2O3)=5.9 moles of Fe
2x= 5.9
x=2.95 moles( 159.7 g/ 1 mole of Fe2O3)
=4.71 x 10 ^2 grams of Fe2O3.