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Using the equation, $Fe_2O_3 + 2Al -> 2Fe + Al_2O_3$, how many grams of $Al$ are needed to completely react with 135 grams of $Fe_2O_3$?
The coefficients in the equation provide a molar ratio between the chemical species in the equation, so you must first convert the mass of iron (III) oxide to moles of...
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Iron is extracted from iron ore. Part of the process involves reduction of the ore with carbon monoxide. Iron ore contains iron oxide ($Fe_2O_3$). How would you write a balanced equation for the reaction of iron oxide with carbon monoxide?
And this is the effectual chemical reaction of our civilization. If you ever have a chance to tour a blast furnace (and most are in China and India now) do...
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How many grams of $Fe_2O_3$ are there in 0.500 mole of $Fe_2O_3$?
Assume that: n = number of moles m = mass of substance M = molar mass (equivalent to atomic weight on the periodic table) $n = m -: M$...
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What is the percentage by mass of iron (Fe) in the mineral hematite ($Fe_2O_3$)?
First find the total mass of the compound $ 3xx 15.999 = 48 $ grams for Oxygen $ 2 xx 55.8 = 111.6$ grams for Iron adding these...
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How many moles of iron, $Fe$, can be made from $Fe_2O_3$ by the use of 18 moles of carbon monoxide, $CO$ in the reaction $Fe_2O_3 + CO -> Fe+CO_2$?
The given equation takes the following form when balanced $Fe_2O_3+3CO=2Fe+3CO_2$ This equation reveals that 2moles of Fe is produced when 3moles of CO reacts Hence 18 moles of CO can...
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If 2.112 g of $Fe_2O_3$ reacts with 0.687 g of $Al$, how much pure $Fe$ will be produced in the reaction $Fe_2O_3(s) + 2Al(s) -> Al_2O_3(s) + 2Fe(s)$?
$"Moles of ferric oxide"=(2.112*g)/(159.69*g*mol^-1)$ $=$ $0.0132*mol$ $"Moles of aluminum"=(0.687*g)/(26.98*g*mol^-1)$ $=$ $0.0254*mol$ Aluminum is in slight deficiency, and is thus the . So $0.0254*molxx55.85*g*mol^-1=1.42*g$. I should add that there is a...
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Iron (III) oxide reacts with carbon monoxide to form molten iron and carbon dioxide. If .18 g of iron (III) oxide reacts with 0.11 g of carbon monoxide, how many grams of iron would be produced?
$"Moles of ferric oxide "=(0.18*g)/(159.69*g*mol^-1)$ $=$ $1.13xx10^-3*mol" metal oxide"$. $"Moles of carbon monoxide "=(0.11*g)/(28.0*g*mol^-1)$ $=$ $3.93xx10^-3*mol" CO"$. $Fe_2O_3$ is the reagent in deficiency (why?), and thus $2xx1.13xx10^-3*molxx55.85*g*mol^-1~=0.150*g$ iron metal are...
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What mass of carbon dioxide is produced by the reduction of $Fe_2O_3$ by carbon monoxide?
$Fe_2O_3(s) + 3CO(g) + Delta rarr 2Fe(l) + 3CO_2(g)uarr$ For each mole of ferric oxide, 3 moles of carbon dioxide are produced. So $"Moles of ferric oxide" = (100*g)/(159.69*g*mol^-1)$...
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Combining 0.265 mol of $Fe_2O_3$ with excess carbon produced 14.7 g of Fe. $Fe_2O_3 + 3C -> 2Fe +3CO.$ What is the actual yield of iron in moles?
You have the chemical equation, which shows that each mole of ferric oxide should yield 2 moles of iron metal: $Fe_2O_3(s) + 3C(s) rarr 2Fe(l) + 3CO(g)$ $"Moles of iron"$...
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Oxygen almost always has an oxidation number of -2. Therefore in the formula for the mineral wüstite, $FeO$, what must the oxidation number for iron be? In the formula for hematite, $Fe_2O_3$, what must the oxidation number for iron be?
In its oxides, an oxidation number of $-II$ is typical. And since, for neutral , the sum of the is $0$. For $"ferrous oxide"$ we have $Fe^(+II)O^(-II)$; and for $"ferric...
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