Calculate the number of grams of Fe formed when 0.300kg of Fe2O3 reacts.
Equation:
Fe2O3+CO-->Fe+CO2
converted .300kg to 300g
Balanced Fe2O3+3CO-->2Fe+3CO2
So I started by trying this:
300gFe2O3(1molFe2O3/159.687gFe2O3)...and then I don't know where I would go from there. I'm not even sure if I'm even starting off right. I'm trying to follow along with the teacher's notes, but she didn't have anthing like this.
how many moles of Fe2O3 do you have? figure that.
Then, the balanced equation tells you that you get twice that number of moles of Fe.
as your teacher did, then
300gFe2O3(1molFe2O3/159.687gFe2O3)*2moleFe/1moleFe2O3
Yeah, I balanced it already; I put it up. My teacher didn't do this, that's why I didn't know how to start, but is that pretty much all I have to do? That extra multiplication/division?
Just to clarify, when I convert from moles to grams, do I double Fe because it has the coefficient 2?
Well, let's figure this out together, shall we?
You've started off correctly by converting the mass of Fe2O3 to grams.
To continue, we can use the balanced equation to determine the molar ratio between Fe2O3 and Fe.
According to the equation Fe2O3 + 3CO -> 2Fe + 3CO2, we see that 1 mole of Fe2O3 reacts to produce 2 moles of Fe.
So, now we can set up the conversion:
300g Fe2O3 x (1 mol Fe2O3/159.687g Fe2O3) x (2 mol Fe/1 mol Fe2O3) x (55.845g Fe/1mol Fe)
Let's break it down:
The molar mass of Fe2O3 is 159.687g/mol, so we use the conversion 1 mol Fe2O3/159.687g Fe2O3.
The molar ratio between Fe2O3 and Fe is 2 moles Fe/1 mole Fe2O3.
Finally, the molar mass of Fe is 55.845g/mol, so we use the conversion 55.845g Fe/1 mol Fe.
By multiplying these conversions together, we can find the answer:
300g Fe2O3 x (1 mol Fe2O3/159.687g Fe2O3) x (2 mol Fe/1 mol Fe2O3) x (55.845g Fe/1mol Fe) ≈ 208.828g Fe
So, approximately 208.828 grams of Fe would be formed when 0.300kg of Fe2O3 reacts.
Hope that helps!
To solve this problem, you are on the right track with converting the mass of Fe2O3 to moles. Let's proceed step by step:
1) First, convert the mass of Fe2O3 from grams to moles. You can do this by using the molar mass (159.687 g/mol) of Fe2O3:
300 g Fe2O3 * (1 mol Fe2O3 / 159.687 g Fe2O3) = 1.8787 mol Fe2O3
2) Now that you have the moles of Fe2O3, you need to determine the stoichiometric ratio between Fe2O3 and Fe. From the balanced equation, you know that 1 mole of Fe2O3 produces 2 moles of Fe:
1.8787 mol Fe2O3 * (2 mol Fe / 1 mol Fe2O3) = 3.7574 mol Fe
3) Finally, to calculate the mass of Fe formed, you can multiply the number of moles of Fe by its molar mass (55.845 g/mol):
3.7574 mol Fe * (55.845 g Fe / 1 mol Fe) = 209.77 g Fe
Therefore, when 0.300 kg (300 g) of Fe2O3 reacts, approximately 209.77 grams of Fe are formed.