# AP chem!!!

Iron ore consists mainly of iron III oxide. When iron III oxide is heated with an excess of coke(carbon), iron metal and carbon monoxide are produced. Assume that even if an excess of coke is not present that the reaction proceeds as described.

A)write a balanced equation for the above reaction.

B) If you started with 3.19g of iron III oxide and 1.00g of coke, how many grams of carbon monoxide would you theoretically obtain?

C. what is the limiting reactant????

D. if you only obtained 1.25g of carbon monoxide, what is your percent yield for this reaction?

Iron ore consists mainly of iron III oxide. When iron III oxide is heated with an excess of coke(carbon), iron metal and carbon monoxide are produced. Assume that even if an excess of coke is not present that the reaction proceeds as described.

A)write a balanced equation for the above reaction.
Fe2O3 + 3C ==> 2Fe + 3CO

B) If you started with 3.19g of iron III oxide and 1.00g of coke, how many grams of carbon monoxide would you theoretically obtain? see below

C. what is the limiting reactant????
Answered in the details of step b below.

D. if you only obtained 1.25g of carbon monoxide, what is your percent yield for this reaction?
Theoretical yield is the number from part b above (which is step 4 in the details below).
%yield = [1.25g/theoretical] x 100 = ??

For (b)This is a limiting reagent problem.
Step 1. Write a balanced equation. That is done.

Step 2. Convert what you have (in this case Fe2O3 and C) to mols. Remember mols = g/molar mass
2a. mols Fe2O3=3.19/molar mass Fe2O3.
2b. mols C = 1.00g/molar mass C.

Step 3. Using the coefficients in the balanced equation, convert mols of what you have (Fe2O3 and C) to mols of what you want (in this case CO).
3a. from Fe2O3. ??mols Fe2O3 x (3 mols CO/1 mol Fe2O3)= xx mols CO.
3b. from C. ??mols C x (3 mols CO/3 mols C) = yy mols CO.
3c. Obviously, both answers can't be correct so you must determine which (either 3a or 3b) it is. The correct answer will always be the smaller of 3a or 3b. That is the limiting reagent and that will be the number used for the next step.

Step 4. Convert mols CO to grams. Just reverse step 2 above. That is mols = g/molar mass; therefore, mols x molar mass = grams.

Post your work if you get stuck. I hope this helps.

1. 👍
2. 👎
3. 👁

## Similar Questions

1. ### Chemistry

Write skeleton equations for these reactions. a. hydrogen iodide(g) --> hydrogen(g) + iodine(g) b. aluminum(s)+iodine(s)--> aluminum iodide(s) c. iron(II) oxide(s) + oxygen(g) --> iron(III) oxide(s)

2. ### Chemestry

Iron metal reacts with oxygen gas to form rust, iron (III) oxide. Which of the following correctly shows the balanced equation for this reaction?

3. ### Chemistry-Equations

Iron(III) oxide is formed when iron combines with oxygen in the air. How many grams of Fe2O3 are formed when 16.7 g of Fe reacts completely with oxygen?

4. ### chemistry

Iron reacts with chlorine to form iron(iii)chloride. A)How many chlorines react with 1.86g of iron? B)What mass of iron(iii)chloride is produced?

1. ### chemistry

iron(III) oxide reacts with carbon monoxide gas to form solid iron metal and carbon dioxide gas: Fe2O3 + 3 CO --> 2 Fe + 3 CO2 If you begin the reaction with 84.34 g of iron(III) oxide and 68.87 g of CO, which reactant will be in

2. ### stoichiometry

When aluminum is mixed with iron(III) oxide, iron metal and aluminum oxide are produced along with a large quantity of heat. Fe2O3(s) + 2 Al(s) 2 Fe(s) + Al2O3(s) + heat What mole ratio would you use to determine moles Fe if moles

3. ### Chemistry-Equation

When iron rusts in air, iron(III) oxide is produced. How many moles of oxygen react with 2.4 mol of iron in the rusting reaction?

4. ### Chemistry

When iron (Fe) rusts (reacts with O2), the product is iron(III) oxide (Fe2O3). If 25 g Fe is reacted with 25 g O2 in a sealed container, what are the masses of Fe, O2 and Fe2O3 in the container after the reaction is complete? How

1. ### Chemistry

When 84.8 g of iron(III) oxide reacts with an excess of carbon monoxide, iron is produced. Fe2O3(s) + 3CO(g) ==> 2Fe(s) + 3CO2(g) what is the theoretical yield of iron?

2. ### chemistry SERIOUS HELP N PROOFREADING

ok it says give the formula for this one Hydronitric acid, I put H3N For Iron (III) chloride I put Fe3Cl Silver acetrate i put AG1C2 Ca(OH02 i put calcium oxide for CCL4 I had no clue Mercury (II) oxide i put HG2O NaClO3 I put

3. ### Last Question Plz helppp:((im soo sleepy!!:(

1)The reaction between solid sodium and iron(III) oxide, Fe2O3(s), is one in a series of reactions that occurs when an automobile air bag inflates. 6Na(s) + Fe2O3(s) -> 3Na2o(s) + 2Fe(s) If 100.0 g of iron(III) oxide are used in

4. ### Chemistry

How many grams of iron can be obtained from a 268 g sample of iron (III) oxide (Fe^2 O^3)?