When iron metal reacts with oxygen, the reaction can form Fe203. The balanced chemical equation I think is right is 4 Fe + 302----2Fe203. So I have 4 moles of iron + 3 moles of oxygen creates 2 moles of iron oxide. I need to find the number of moles of oxygen that are needed to form 6 mol of Fe203. Could you show all work so I can understand?

do it as a proportion:

6molFe2O3/2molFe2O3 as ?/3molO2
?=9molesO2

Sure! To find the number of moles of oxygen needed to form 6 moles of Fe203, we can use the balanced chemical equation:

4 Fe + 3 O2 → 2 Fe203

According to the equation, 3 moles of oxygen is required to react with 4 moles of iron to produce 2 moles of iron oxide. This means that for every 2 moles of Fe203, we need 3 moles of oxygen.

Now, we can set up a proportion to solve for the number of moles of oxygen needed:

(3 moles O2 / 2 moles Fe203) = (x moles O2 / 6 moles Fe203)

Cross-multiplying we get:

3 moles O2 * 6 moles Fe203 = 2 moles Fe203 * x moles O2

18 moles O2 = 2x

Dividing both sides by 2:

x = 18 moles O2 / 2

x = 9 moles O2

So, 9 moles of oxygen are needed to form 6 moles of Fe203.

Sure! To find the number of moles of oxygen needed to form 6 mol of Fe203, we can use the balanced chemical equation you provided.

The equation states that 4 moles of iron react with 3 moles of oxygen to produce 2 moles of iron oxide (Fe203).

We can set up a proportion to find the number of moles of oxygen needed:

(4 moles Fe) / (3 moles O2) = (2 moles Fe203) / (x moles O2)

Here, we know the number of moles of iron (Fe) is 4 and the number of moles of iron oxide (Fe203) is 2. We need to find the number of moles of oxygen (O2), which is represented by 'x'.

Now, we can solve for 'x' by cross-multiplying:

4 moles Fe * x moles O2 = 3 moles O2 * 2 moles Fe203

4x = 6

Dividing both sides by 4, we get:

x = 6/4

x = 1.5

Therefore, to form 6 mol of Fe203, you would need 1.5 moles of oxygen (O2).