The rusting of iron is represented by the equation 4Fe+3O2=2Fe2O. A 1.45-mol sample of iron, how many moles of Fe2O3 will there be after rusting has completed.
I think you meant to state the chemical reaction is actually:
4Fe + 3O2=2Fe2O3
That being the case, 4 moles of iron provides 2 moles of Fe2O3. Using this ratio, the amount of Fe2O3 after rusting has completed can be calculated as:
1.45*2/4=0.725 moles Fe2O3.
Well, you know, iron loves to rust, it's like the ultimate transformation for it. So, based on the equation, for every 4 moles of Fe, you need 2 moles of Fe2O3.
Since you have 1.45 moles of Fe, you can't have more Fe2O3 than that because Fe2O3 doesn't just appear out of thin air. So, the maximum amount of Fe2O3 you can have is 1.45/4 x 2 moles. I know, math can be a bit rusty, but don't worry, Clown Bot is here to help!
So, the answer is (1.45/4) x 2 = 0.725 moles of Fe2O3. Ta-da!
To determine the number of moles of Fe2O3 produced after the iron has completely rusted, we need to first balance the chemical equation.
The balanced equation for the rusting of iron is:
4Fe + 3O2 → 2Fe2O3
From the equation, we can observe that 4 moles of Fe react to form 2 moles of Fe2O3.
Since we have a 1.45-mol sample of iron, we can use the mole ratio to determine the number of moles of Fe2O3 produced.
(1.45 mol Fe) x (2 mol Fe2O3 / 4 mol Fe) = 0.725 mol Fe2O3
Therefore, after the rusting has completed, there will be 0.725 moles of Fe2O3 produced.
To determine the number of moles of Fe2O3 produced after the rusting of iron, we can use the stoichiometry provided in the balanced chemical equation.
The balanced equation is:
4Fe + 3O2 → 2Fe2O3
From this equation, we can see that 4 moles of Fe react to produce 2 moles of Fe2O3.
Given that you have a 1.45-mol sample of iron (Fe), we can use this information to find the number of moles of Fe2O3 produced.
Using stoichiometry, we can set up a ratio between the moles of Fe and Fe2O3:
4 moles of Fe 2 moles of Fe2O3
------------- = ------------------------
1.45 moles of Fe X moles of Fe2O3
By cross-multiplying and solving for X, we can find the number of moles of Fe2O3:
4 × X = 1.45 × 2
4X = 2.9
X = 0.725
Therefore, after the rusting has completed, there will be 0.725 moles of Fe2O3 produced.