Skip to main content
Pearson+ LogoPearson+ Logo
Ch.4 - Chemical Quantities & Aqueous Reactions
Back
Previous problem
Next problem
All textbooksTro 4th EditionCh.4 - Chemical Quantities & Aqueous ReactionsProblem 124

Chapter 4, Problem 124

An important reaction that takes place in a blast furnace during the production of iron is the formation of iron metal and CO2 from Fe2O3 and CO. Determine the mass of Fe2O3 required to form 910 kg of iron. Determine the amount of CO2 that forms in this process.

Verified Solution
Video duration:
0m:0s
This video solution was recommended by our tutors as helpful for the problem above.
2656
views
2
rank
Was this helpful?

Video transcript

Hello everyone. Today, we have the following problem. An important reaction that takes place in a blast furnace during the production of iron is the formation of iron metal and carbon dioxide from ferrous oxide and carbon monoxide determine the mass of the ferrous oxide required to form 910 kg of iron, determine the amount of carbon dioxide that forms in this process. So if we were to write out the equation for this reaction, we would have our ferrous oxide which is a solid reacting with our carbon monoxide, which is a gas to form the fallen. We would have our iron which is a solid and then we would have our carbon dioxide which is a gas. So we see that it is already balanced. So we can proceed with the second part of our question. So to find the mass of our ferrous oxide, we start out with what we were given which was 910 kg. However, we will convert this 1st 2 g and we simply use the conversion factor that 1 kg is equal to 10 to the third grams to get 9.1 times 10 to the fifth grams of iron. Now we can multiply by the molar mass, which states that one mole of iron is equal to 55.845 g. From that conversion, we can then multiply by the multiple ratio between iron and and ferrous oxide in that when we had our reaction and we, we reacted one mole of our ferrous oxide. If we look at the subscript of the iron, we see that it is two. That means we used two moles of iron. In that process, we then can finally use the molar mass of our ferrous oxide and convert back to our kilograms. And so we do that. And so to do that, we first multiply by the molar mass which is one mole of our ferrous oxide multiplied by the molar mass which is 160 g. And then we can multiply back to fine grams with the conversion factor that 10 rates to the power of 3 g is equal to 1 kg. When our units cancel out, we end up with a mass of 1.3 times 10 to the third kilograms of our ferris oxy. Now we can find them all. I could find the mass of our carbon dioxide. We also use what we were given which was 9.1 times 10 to the fifth grams of iron. We multiply by the same molar mass of iron, which is one mole of iron is equal to the 55 points, 8 4 5 g. And then we multiply by a multiple ratio this time using moles of iron to carbon dioxide. So once again, we had two moles of iron involved in the process. And for carbon dioxide, we would actually have three moles of this. We then multiply by the same conversion factor to get back to kilograms, which is 10 race 10 erase the power of 3 g is equal to 1 kg. And then we should also include our molar mass of carbon dioxide which states that one mole is equal to 44 0.01 g. When our units canceled out, we will get a mass of 1.08 times 10 to the negative 3 kg of carbon dioxide. And if you look at wa as we see the tra B best reflects this overall, I hope is helped. And until next time.
Previous problemNext problem
Related Practice
Textbook Question

A solution contains one or more of the following ions: Hg22+ , Ba2+ , and Fe2+ . When you add potassium chloride to the solution, a precipitate forms. The precipitate is filtered off, and you add potassium sulfate to the remaining solution, producing no precipitate. When you add potassium carbonate to the remaining solution, a precipitate forms. Which ions were present in the original solution?

1417
views
Textbook Question

A solution contains one or more of the following ions: Hg2 2 + , Ba2 + , and Fe2 + . When you add potassium chloride to the solution, a precipitate forms. The precipitate is filtered off, and you add potassium sulfate to the remaining solution, producing no precipitate. When you add potassium carbonate to the remaining solution, a precipitate forms. Write net ionic equations for the formation of each of the precipitates observed.

842
views
Textbook Question

The reaction of NH3 and O2 forms NO and water. The NO can be used to convert P4 to P4O6, forming N2 in the process. The P4O6 can be treated with water to form H3PO3, which forms PH3 and H3PO4 when heated. Find the mass of PH3 that forms from the reaction of 1.00 g of NH3.

2337
views
Textbook Question

A liquid fuel mixture contains 30.35% hexane (C6H14), 15.85% heptane (C7H16), and the rest octane (C8H18). What maximum mass of carbon dioxide is produced by the complete combustion of 10.0 kg of this fuel mixture?

3191
views
Textbook Question

Titanium occurs in the magnetic mineral ilmenite (FeTiO3), which is often found mixed with sand. The ilmenite can be separated from the sand with magnets. The titanium can then be extracted from the ilmenite by the following set of reactions: FeTiO3(s) + 3 Cl2( g) + 3 C(s)¡3 CO(g) + FeCl2(s) + TiCl4( g) TiCl4( g) + 2 Mg(s)¡2 MgCl2(l ) + Ti(s) Suppose that an ilmenite–sand mixture contains 22.8% ilmenite by mass and that the first reaction is carried out with a 90.8% yield. If the second reaction is carried out with an 85.9% yield, what mass of titanium can be obtained from 1.00 kg of the ilmenite– sand mixture?

1868
views