Is this correct?
When iron metal reacts with oxygen, the reaction can form Fe2O3. Write a balanced chemical equation for this reaction, and find the number of moles of oxygen that are needed to form 6 mol of Fe2O3. Show your work.
4Fe + 3O2---> 2Fe2O3
9moles of O2 are needed to produce 6mol of Fe2O3 since the ratio of oxygen to iron(II)oxide is 3:2
Yes.
Yes, your balanced chemical equation is correct:
4Fe + 3O2 → 2Fe2O3
To find the number of moles of oxygen needed to form 6 mol of Fe2O3, we can use the mole ratio between oxygen and Fe2O3 from the balanced equation. The ratio of oxygen to Fe2O3 is 3:2.
Given that 6 mol of Fe2O3 is formed, we can set up a ratio:
3 mol O2 / 2 mol Fe2O3 = x mol O2 / 6 mol Fe2O3
Cross-multiplying and solving for x, we get:
3 * 6 = 2 * x
18 = 2x
x = 9
Therefore, 9 moles of O2 are needed to form 6 mol of Fe2O3.
Yes, your balanced chemical equation is correct:
4Fe + 3O2 ---> 2Fe2O3
To find the number of moles of oxygen needed to form 6 mol of Fe2O3, we need to compare the stoichiometric ratio of oxygen to Fe2O3 in the balanced equation. Based on the balanced equation, for every 2 moles of Fe2O3, we need 3 moles of O2.
So, to find the number of moles of O2 required for 6 mol of Fe2O3, we can set up a proportion:
(3 moles O2 / 2 moles Fe2O3) = (x moles O2 / 6 moles Fe2O3)
Cross-multiplying, we get:
3 * 6 = 2 * x
18 = 2x
Dividing both sides by 2, we find:
x = 9
Therefore, 9 moles of O2 are needed to produce 6 mol of Fe2O3.