how many moles of iron would have been used up if 45.0g of copper were to be produced?
is it # mols Fe = 45.0gCu x 1mol/63.5g = 0.709molFe ?
lmfao im here in 2021 at 12:05am trying to understand moles for my test wooo
Wouldn't it depend on the reaction?
copper produced from iron + copper II chloride
nevermind i get it now, i can find the answer with the
moles of copper produced/moles of iron used ratio
thanks
Well, I must say that would be quite a talent for iron to transform itself into copper! But alas, iron cannot just disappear into thin air... or should I say, thin mol.
To answer your question, the equation seems to be incorrect. The molar mass of copper (Cu) is indeed 63.5 g/mol, but there is no direct relationship between copper and iron (Fe) in the equation you mentioned.
In order to determine the moles of iron used, we need to know the balanced chemical equation for the reaction that produces copper.
Yes, you have correctly calculated the number of moles of iron that would have been used up if 45.0g of copper were to be produced.
To determine the number of moles of iron used, you can use the concept of stoichiometry. The balanced chemical equation for the reaction that produces copper from iron is:
2 Fe + CuSO4 -> Cu + Fe2(SO4)3
According to the equation, 2 moles of iron react to produce 1 mole of copper. This means that the mole ratio between iron and copper is 2:1.
Now, you can use this mole ratio to calculate the number of moles of iron used. You are given the mass of copper (45.0g), and you need to convert it to moles using the molar mass of copper (63.5g/mol).
45.0g Cu x (1 mol Cu/63.5g Cu) = 0.709 mol Cu
Since the mole ratio of iron to copper is 2:1, the number of moles of iron used would be half of the moles of copper:
0.709 mol Cu x (1 mol Fe/2 mol Cu) = 0.354 mol Fe
So, the correct answer is 0.354 mol Fe, not 0.709 mol Fe.
The balanced equation is ...
2Fe + 3CuCl2 >> 2FeCl3 + 3Cu
45gCu*63.5gCu/molCu*2molesFe/3molesCu