Iron metal reacts with oxygen gas to produce iron(III) oxide. If you have 12.0 moles of iron, for complete reaction you need:
(HINT you need the balanced chemical reaction!)
A) 9.0 moles of O2 and produce 3.0 moles of Fe2O3
B) 9.0 moles of O2 and produce 6.0 moles of Fe2O3
4Fe + 3O2>> 2Fe2O3
Looks like a 3:2 ratio to me.
To determine the number of moles of oxygen gas (O2) needed for the complete reaction, we first need to write the balanced chemical equation for the reaction:
4Fe + 3O2 → 2Fe2O3
The balanced equation tells us that 4 moles of iron (Fe) react with 3 moles of oxygen gas (O2) to produce 2 moles of iron(III) oxide (Fe2O3).
Now, we have 12.0 moles of iron (Fe). We can set up a ratio using the stoichiometric coefficients from the balanced equation:
4 moles of Fe : 3 moles of O2
Since we have 12.0 moles of Fe, we can solve for the moles of O2 as follows:
12.0 moles Fe * (3 moles O2 / 4 moles Fe) = 9.0 moles O2
Therefore, the correct answer is A) 9.0 moles of O2 and it will produce 3.0 moles of Fe2O3.
To determine the number of moles of oxygen gas (O2) and iron(III) oxide (Fe2O3) required for the complete reaction with 12.0 moles of iron (Fe), we need to look at the balanced chemical equation for the reaction.
The balanced chemical equation for the reaction between iron and oxygen is:
4 Fe + 3 O2 -> 2 Fe2O3
From the balanced equation, we can see that:
- 4 moles of Fe react with 3 moles of O2 to produce 2 moles of Fe2O3.
Therefore, to find the amount of O2 required for 12.0 moles of Fe, we can set up a simple proportion:
(12.0 moles Fe / 4 moles Fe) = (x moles O2 / 3 moles O2)
Cross-multiplying and solving for x:
12.0 moles Fe * 3 moles O2 = 4 moles Fe * x moles O2
36 moles O2 = 4x
x = 36 moles O2 / 4
x = 9 moles O2
So, for the complete reaction of 12.0 moles of Fe, you would need 9.0 moles of O2.
Next, let's determine the amount of Fe2O3 produced. From the balanced equation, we can see that:
- 4 moles of Fe react to produce 2 moles of Fe2O3.
So, for every 4 moles of Fe, we get 2 moles of Fe2O3. Using the same proportion method:
(12.0 moles Fe / 4 moles Fe) = (x moles Fe2O3 / 2 moles Fe2O3)
Cross-multiplying and solving for x:
12.0 moles Fe * 2 moles Fe2O3 = 4 moles Fe * x moles Fe2O3
24 moles Fe2O3 = 4x
x = 24 moles Fe2O3 / 4
x = 6 moles Fe2O3
Therefore, for the complete reaction of 12.0 moles of Fe, you would produce 6.0 moles of Fe2O3.
In conclusion, for the complete reaction of 12.0 moles of Fe, you would need:
B) 9.0 moles of O2 and produce 6.0 moles of Fe2O3.