Iron(III) oxide is formed when iron combines with oxygen in the air. What is the mole ration of Fe used and the mole of Iron(iii) oxide produced? 4Fe(s) + 3O2(g) > 2Fe2O3(s)

a - 3:2
b - 4:3
c - 4:2
d - 3:4

Can someone help?

This is quite simple. The coefficients tell you what is going on. The equation tells you that 4 mols Fe react with 3 mols O2 to produce 2 mols Fe2O3.

So the ratio of Fe used (4 mols) to iron(III) oxide produced(2 mols) is 4:2. right. In other words, mols Fe2O3 produced is just 1/2 that of Fe used.

Sure! To determine the mole ratio of Fe used and the mole of Iron(III) oxide produced, we need to look at the balanced chemical equation:

4Fe(s) + 3O2(g) -> 2Fe2O3(s)

From the equation, we can see that for every 4 moles of Fe used, 2 moles of Fe2O3 are produced. Therefore, the mole ratio of Fe used to Fe2O3 produced is 4:2, which simplifies to 2:1.

Comparing this with the answer choices provided:
a - 3:2
b - 4:3
c - 4:2
d - 3:4

We can see that the correct answer is c - 4:2 (which is equivalent to 2:1).

So the mole ratio of Fe used to Fe2O3 produced is 2:1.