Question

In the oxidation of Iron Sulfide (FeS2) where Ferric oxide (Fe2O3) and sulfur dioxide (SO2) are...

In the oxidation of Iron Sulfide (FeS2) where Ferric oxide (Fe2O3) and sulfur dioxide (SO2) are formed; 100 g of FeS2 and 100 g of O2 are introduced. Determine:

The balanced reaction.
Limiting reagent and excess reagent.

Engineering   Chemical-Engineering   
0 0
Add a commentTranscribed image text
Next >

Homework Answers

Answer #1

0 0
Know the answer?
Your Answer:

Post as a guest

Your Name:

What's your source?

Earn Coins

Coins can be redeemed for fabulous gifts.

Log In

Sign Up

Not the answer you're looking for?
Ask your own homework help question
Similar Questions
Hydrogen sulfide gas is used to precipitate the ferric ion from solution as the sulfide salt....
Hydrogen sulfide gas is used to precipitate the ferric ion from solution as the sulfide salt. In a particular reaction, 4.000 L of H2S gas at STP is bubbled into 85.00 mL of a 1.400 M Solution of ferric chloride. What is the mass of ferric sulfide formed? Determine the moles of the reagent not completely consumed. 2Fe^3+(aq) + 3H2S(g) --> Fe2S3(s) + 6H^+(aq) (balanced) MM of Fe2S3 is 207.88 g/mol.
∆Ho = −3310 kJ/mol for: 4 FeS2(s) + 11 O2(g) → 2 Fe2O3(s) + 8 SO2(g)...
∆Ho = −3310 kJ/mol for: 4 FeS2(s) + 11 O2(g) → 2 Fe2O3(s) + 8 SO2(g) If ∆Hof [Fe2O3(s)] = -824.2 and ∆Hof [SO2(g)] = −296.83 kJ/mol determine ∆Ho for Fe(s) + 2S(s) → FeS2(s).
When lead(II) sulfide reacts with oxygen (O2) gas, the products are lead(II) oxide and sulfur dioxide...
When lead(II) sulfide reacts with oxygen (O2) gas, the products are lead(II) oxide and sulfur dioxide gas.How many grams of lead(II) sulfide are used to produce 129 g of lead(II) oxide?
When lead(II) sulfide reacts with oxygen (O2) gas, the products are lead(II) oxide and sulfur dioxide...
When lead(II) sulfide reacts with oxygen (O2) gas, the products are lead(II) oxide and sulfur dioxide gas.How many grams of oxygen are required to react with 25.1 g of lead(II) sulfide?
When coal is burned, the sulfur it contains is converted into sulfur dioxide. This SO2 is...
When coal is burned, the sulfur it contains is converted into sulfur dioxide. This SO2 is a serious pollutant, so it needs to be removed before it escapes from the stack of a coal fired plant. One way to remove the SO2 is to add limestone, which contains calcium carbonate, CaCO3, to the coal before it is burned. The heat of the burning coal converts the CaCO3 to calcium oxide, CaO. The calcium oxide reacts with the sulfur dioxide in...
When coal is burned, the sulfur it contains is converted into sulfur dioxide. This SO2 is...
When coal is burned, the sulfur it contains is converted into sulfur dioxide. This SO2 is a serious pollutant, so it needs to be removed before it escapes from the stack of a coal fired plant. One way to remove the SO2 is to add limestone, which contains calcium carbonate, CaCO3, to the coal before it is burned. The heat of the burning coal converts the CaCO3 to calcium oxide, CaO. The calcium oxide reacts with the sulfur dioxide in...
When coal is burned, the sulfur it contains is converted into sulfur dioxide. This SO2 is...
When coal is burned, the sulfur it contains is converted into sulfur dioxide. This SO2 is a serious pollutant, so it needs to be removed before it escapes from the stack of a coal fired plant. One way to remove the SO2 is to add limestone, which contains calcium carbonate, CaCO3, to the coal before it is burned. The heat of the burning coal converts the CaCO3 to calcium oxide, CaO. The calcium oxide reacts with the sulfur dioxide in...
For the following reaction, 23.1 grams of sulfur dioxide are allowed to react with 9.19 grams...
For the following reaction, 23.1 grams of sulfur dioxide are allowed to react with 9.19 grams of oxygen gas . sulfur dioxide(g) + oxygen(g) sulfur trioxide(g) What is the maximum mass of sulfur trioxide that can be formed? grams What is the FORMULA for the limiting reagent? What mass of the excess reagent remains after the reaction is complete? Please show your work I am having a very hard time trying to understand these problems.
The balanced equation for the reaction of iron (III) oxide with carbon monoxide to produce carbon...
The balanced equation for the reaction of iron (III) oxide with carbon monoxide to produce carbon dioxide and iron metal is given below. Fe2O3 (s) + 3 CO (g) --> 2 Fe (s) + 3 CO2 (g) Using the balanced equation, determine the mass of iron metal (Fe(s)) in grams that can be made if this reaction is performed using 225.3 grams of iron (III) oxide (Fe2O3) and 200.1 grams of carbon monoxide.
Iron reacts with oxygen at high temperatures to form iron(III) oxide. 4Fe(s)+3O2(g)⟶2Fe2O3(s)4Fe(s)+3O2(g)⟶2Fe2O3(s) Suppose 12.3 g12.3 g...
Iron reacts with oxygen at high temperatures to form iron(III) oxide. 4Fe(s)+3O2(g)⟶2Fe2O3(s)4Fe(s)+3O2(g)⟶2Fe2O3(s) Suppose 12.3 g12.3 g of iron (Fe)(Fe) is reacted with 21.0 g21.0 g of oxygen (O2).(O2). Select the limiting reagent. FeFe Fe2O3Fe2O3 O2O2 Calculate the theoretical yield of iron(III) oxide (Fe2O3Fe2O3). theoretical yield = g The reaction produces 5.63 g5.63 g of Fe2O3.Fe2O3. What is the percent yield of the reaction? percent yield =
ADVERTISEMENT
Need Online Homework Help?

Get Answers For Free
Most questions answered within 1 hours.

Ask a Question
ADVERTISEMENT