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. Be sure your equation is balanced.
Given :
2C (s) + O2 (g) → 2CO (g) ....eqn 1
Fe2O3 (s) + 3CO (g) → 2Fe (s) + 3CO2 (g) ...eqn 2
Multiply eqn 1 by 3 and eqn 2 by 2 to get below
eqns,
6C (s) + 3O2 (g) → 6CO (g) .... eqn 3
2Fe2O3 (s) + 6CO (g) → 4Fe (s) + 6CO2 (g) ...eqn 4
Now add eqn 3 and eqn 4 to get the desired
equation:
6C (s) + 3O2 (g) + 2Fe2O3 (s) → 4Fe (s) + 6CO2 (g)
Blast furnaces extract pure iron from the iron(III) oxide in iron ore in a two step...
Iron metal is made from iron ore in a blast furnace, were this chemical reaction occurs: Fe2O3(s) + 3CO(g) --> 2Fe(s) + 3CO2(g) (a) Is this a redox equation? State why it is or why it is not. (b) If 175 kg of iron ore (Fe2O3) is reacted with excess carbon monoxide (CO), what is the theoretical yield (amount in kg) of iron metal (Fe)? (c) If the actual yield of iron metal is 109 kg, what is the percent...
Iron metal is made from iron ore in a blast furnace, were this chemical reaction occurs: Fe2O3(s) + 3CO(g) --> 2Fe(s) + 3CO2(g) (a) Is this a redox equation? State why it is or why it is not. (b) If 175 kg of iron ore (Fe2O3) is reacted with excess carbon monoxide (CO), what is the theoretical yield (amount in kg) of iron metal (Fe)? (c) If the actual yield of iron metal is 109 kg, what is the percent...
Iron metal is made from iron ore in a blast furnace, were this chemical reaction occurs: Fe2O3(s) + 3CO(g) --> 2Fe(s) + 3CO2(g) (a) Is this a redox equation? State why it is or why it is not. (b) If 175 kg of iron ore (Fe2O3) is reacted with excess carbon monoxide (CO), what is the theoretical yield (amount in kg) of iron metal (Fe)? (c) If the actual yield of iron metal is 109 kg, what is the percent...
Iron ore is reduced to pure iron by smelting, during which the iron (III) oxide in the ore reacts with carbon monoxide gas, like this: Fe2O3(s)+3CO(g) → 2Fe (s)+3CO2() Suppose an engineer decides to study the rate of this reaction. She prepares four reaction vessels with 93.4 g of solid iron (III) oxide and 29.8 g of carbon monoxide gas each. The volume and temperature of each vessel is shown in the table below. of reaction. In other words, select...
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?
In a blast furnace, Iron (III) oxide reacts with coke (carbon) to produce molten iron and carbon monoxide. Fe2O3 + 3C = 2Fe + 3CO. How many kg of iron would be formed from 125 kg of Fe2O3?
The balanced equation for the reduction of iron ore to the metal using CO is Fe2O3 (s) + 3CO (g) ----> 2Fe (s) + 3CO2 (g) What is the maximum mass of iron, in grams, that can be obtained from 937 g of iron(III) oxide? Mass = g Fe What mass of CO is required to react with 937 g of Fe2O3? Mass = gCO
When 50.1 g iron(III) oxide reacts with carbon monoxide, 31.7 g iron is produced. What is the percent yield of the reaction? Fe2O3(s)+3CO(g)→2Fe(s)+3CO2(g)
The reduction of iron (III) oxide to iron during steel making can be summarized by this sequence of reaction: K1 2C(s) + O2(g) <--> 2CO(g) K2 Fe2O3(s) + 3CO(g) <--> 2Fe(l) + 3CO2(g) The net reaction is: K = 2Fe2O3(s) + 6C(s) + 3O2(g) <--> 4Fe(l) + 6CO2(g) Write an equation that gives the overall equilibrium constant K in terms of the equilibrium constants K1 and K2 .
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?