Question
A mixture of FeO and Fe2O3 with a mass of 10.0 g is converted to 7.48 g of pure Fe metal. What is the amount of FeO and Fe2O3 (in grams) in the original sample.
Not sure where to start. Any help is appreciated!
Not sure where to start. Any help is appreciated!
Answers
mm = molar mass
am = atomic mass
You have two equations and you solve the two equations simultaneously.
Let X = grams FeO and
let Y = grams Fe2O3.
equation 1 is X + Y = 10.0 g
The second equation is converting this 10.0 g into pure iron in terms of X and Y.
eqn 2 is X(am Fe/mm FeO) + Y(2 am Fe/mm Fe2O3) = 7.48 g
Solve these two equation for X and Y giving you grams FeO and Fe2O3.
Post your work if you get stuck. This is the chem part. The only thing left is the math.
am = atomic mass
You have two equations and you solve the two equations simultaneously.
Let X = grams FeO and
let Y = grams Fe2O3.
equation 1 is X + Y = 10.0 g
The second equation is converting this 10.0 g into pure iron in terms of X and Y.
eqn 2 is X(am Fe/mm FeO) + Y(2 am Fe/mm Fe2O3) = 7.48 g
Solve these two equation for X and Y giving you grams FeO and Fe2O3.
Post your work if you get stuck. This is the chem part. The only thing left is the math.