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?

Md Ariful Islam

0 like 0 dislike
1 views
Share with your friends

1 Answers

Md Ariful Islam

Call

You have the chemical equation, which shows that each mole of ferric oxide should yield 2 moles of iron metal:

$Fe_2O_3(s) + 3C(s) rarr 2Fe(l) + 3CO(g)$

$"Moles of iron"$ $=$ $(14.7*g)/(55.8*g*mol^-1)$ $=$ $0.263*mol$

Because stoichiometric reaction would have yielded $2xx0.265*mol$ of iron metal, the yield of the reaction is just under 50%.

0 like 0 dislike
1 views
Talk Doctor Online in Bissoy App
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...

1 Answers 1 views
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...

1 Answers 1 views
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...

1 Answers 1 views
Iron is obtained commercially by the reaction of hematite $Fe_2O_3$ with carbon monoxide. How many grams of iron is produced when 25.0 mol of hematite reacts with 30.0 mol of carbon monoxide?

As can be seen from the chemical equation, each mole of $Fe_2CO_3$ needs 3 moles of $CO$. If 30 moles of $CO$ are used, only 10 moles of $Fe_2CO_3$ can...

1 Answers 1 views
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...

1 Answers 1 views
In the reaction $Fe_2O_3 + 3CO -> 2Fe + 3CO_2$, what is the total number of moles of $CO$ used to produce 112 grams of iron?

Assume that: n = number of moles m = mass of substance M = molar mass (equivalent to atomic weight in the periodic table) $n = m -: M$ The...

1 Answers 1 views
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...

1 Answers 1 views
Given $Fe_2O_3(s) + 3CO(g) rarr 2Fe(s) + 3CO_2(g)$, how do we calculate the molar equivalence?

$Fe_2O_3(s) + 3CO(g) rarr 2Fe(s) + 3CO_2(g)$ And thus 1 equiv ferric oxide reacts with 3 equiv carbon monoxide to give 2 equiv iron, and 3 equiv carbon dioxide....

1 Answers 1 views
How much iron metal will $160*g$ of ferric oxide provide: $Fe_2O_3(s) + 3C(s) stackrel(Delta)rarr2Fe(s)+3CO(g)$?

$Fe_2O_3 + 3C rarr 2Fe +3COuarr$ Thus 1 mole of ferric oxide gives 2 moles of iron metal upon reduction. Given molar quantities, $160*g$ ferric oxide will provide almost $111*g$...

1 Answers 1 views
Define the terms theoretical yield, actual yield, and percent yield. Why is the actual yield in a reaction almost always less than the theoretical yield? Can a reaction ever have 110% actual yield?

Actual yield in a reaction is almost always less than the theoretical yield, primarily because losses of the substances involved may occur anywhere in an experiment. Otherwise, there can be...

1 Answers 1 views
X