Iron is extracted from iron ore (aka iron(III) oxide) by reacting it with carbon monoxide. Carbon...
Iron is extracted from iron ore (aka iron(III) oxide) by reacting it with carbon monoxide. Carbon dioxide is a by-product of this reaction. Suppose you are involved in the design of a steel plant and are concerned about its environmental impact. You need to know not only the amount of iron you can extract from the ore supplied, but also the amount of carbon dioxide released into the atmosphere during the production. What mass of carbon dioxide (in kg) will be produced in the manufacture 24.0 kg iron? Type your answer to with 3 sig figs and no units.
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Iron is extracted from iron ore (aka iron(III) oxide) by
reacting it with carbon monoxide. Carbon...
Blast furnaces extract pure iron from the iron(III) oxide in iron ore in a two step...
Blast furnaces extract pure iron from the iron(III) oxide in iron ore in a two step sequence. In the first step, carbon and oxygen react to form carbon monoxide: 2C (s) + O2 (g) → 2CO (g) In the second step, iron(III) oxide and carbon monoxide react to form iron and carbon dioxide: Fe2O3 (s) + 3CO (g) → 2Fe (s) + 3CO2 (g) Write the net chemical equation for the production of iron from carbon, oxygen and iron(III) oxide....
5. Iron(III) oxide reacts with carbon monoxide to produce iron and carbon dioxide according to the...
5. Iron(III) oxide reacts with carbon monoxide to produce iron and carbon dioxide according to the following reaction: Fe2O3 + 3 CO → 2 Fe + 3 CO2 a) What is the percent yield of iron if 15.0 grams of FE is actually produced by reacting 65.0 of iron(III) oxide? b) What is the percent yield of carbon dioxide if the reaction produces 85.0 grams of carbon dioxide from 75.0 grams of carbon monoxide?
Write and balance the equation showing the reaction between iron(III) oxide and carbon monoxide to form...
Write and balance the equation showing the reaction between iron(III) oxide and carbon monoxide to form iron metal and carbon dioxide.
Q2) Hematite, Fe2O3, is an important ore of iron. The free metal is obtained by reacting...
Q2) Hematite, Fe2O3, is an important ore of iron. The free metal is obtained by reacting hematite with excess carbon monoxide, CO2, in a blast furnace. Carbon dioxide is formed in the furnace by partial combustion. The unbalanced reaction is: Fe 0; (3) + CO(g) + Fe (8) + CO2(g) How many grams of iron can be produced from placing 1.50 kg of Fe,0, in a blast furnace?
Write and balance the following chemical equations. Iron (III) oxide reacts with carbon monoxide to yield...
Write and balance the following chemical equations. Iron (III) oxide reacts with carbon monoxide to yield iron and carbon dioxide. Rubidium reacts with water to yield rubidium hydroxide and hydrogen. Copper (II) chloride reacts with ammonium phosphate to yield ammonium chloride and copper (II) phosphate. Ammonia and oxygen react to form nitrous oxide (also known as nitrogen monoxide) and water.
Consider the reaction between solid iron(III) oxide and carbon monoxide gas to form carbon dioxide gas...
Consider the reaction between solid iron(III) oxide and carbon monoxide gas to form carbon dioxide gas and solid iron (11,111) oxide. If carbon monoxide is present in excess, determine the amount of iron(III) oxide needed to produce 2.21x1024 iron (11,HI) oxide molecules. O 1.83 moles 3.67 moles 07.34 moles O 11.0 moles O 5.50 moles 0.50 mol A, 0.60 mol B, and 0.90 mol C are reacted according to the following reaction A + 2B + 3C 2D + E...
Iron (III) oxide reacts with carbon monoxide to produce iron and carbon dioxide. Fe2O3(s)+3CO(g)→2Fe(s)+3CO2(g) Part A...
Iron (III) oxide reacts with carbon monoxide to produce iron and carbon dioxide. Fe2O3(s)+3CO(g)→2Fe(s)+3CO2(g) Part A What is the percent yield of iron if the reaction of 67.0 g of iron(III) oxide produces 14.3 g of iron?
A geologist is extracting iron from its ore in a blast furnace. In this process, solid...
A geologist is extracting iron from its ore in a blast furnace. In this process, solid iron(III) oxide is reacted with carbon monoxide, producing molten iron and carbon dioxide. a) Write the complete balanced equation. b) When this reaction is done, the percent yield of pure iron is only 78%. In order to produce 245 kg of iron, how many kilograms of iron(III) oxide I need to start with?
5. Iron(III) oxide reacts with carbon monoxide to produce iron and carbon dioxide according to the following reaction: Fe2O3 + 3 CO → 2 Fe + 3 CO2 a) What is the percent yield of iron if 15.0 grams of FE is actually produced by reacting 65.0 of iron(III) oxide? b) What is the percent yield of carbon dioxide if the reaction produces 85.0 grams of carbon dioxide from 75.0 grams of carbon monoxide?
Q2) Hematite, Fe2O3, is an important ore of iron. The free metal is obtained by reacting hematite with excess carbon monoxide, CO2, in a blast furnace. Carbon dioxide is formed in the furnace by partial combustion. The unbalanced reaction is: Fe 0; (3) + CO(g) + Fe (8) + CO2(g) How many grams of iron can be produced from placing 1.50 kg of Fe,0, in a blast furnace?
Write and balance the following chemical equations. Iron (III) oxide reacts with carbon monoxide to yield iron and carbon dioxide. Rubidium reacts with water to yield rubidium hydroxide and hydrogen. Copper (II) chloride reacts with ammonium phosphate to yield ammonium chloride and copper (II) phosphate. Ammonia and oxygen react to form nitrous oxide (also known as nitrogen monoxide) and water.
Consider the reaction between solid iron(III) oxide and carbon monoxide gas to form carbon dioxide gas and solid iron (11,111) oxide. If carbon monoxide is present in excess, determine the amount of iron(III) oxide needed to produce 2.21x1024 iron (11,HI) oxide molecules. O 1.83 moles 3.67 moles 07.34 moles O 11.0 moles O 5.50 moles 0.50 mol A, 0.60 mol B, and 0.90 mol C are reacted according to the following reaction A + 2B + 3C 2D + E...
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