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Q2) Hematite, Fe2O3, is an important ore of iron. The free metal is obtained by reacting...
Iron metal is made from iron ore in a blast furnace, were this chemical reaction occurs:...
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:...
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:...
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...
The balanced equation for the reduction of iron ore to the metal using CO is Fe2O3 (s)...
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
14. (1 point per blank) Iron ore, Fe2O3 (s), reacts with C (s) in a blast...
14. (1 point per blank) Iron ore, Fe2O3 (s), reacts with C (s) in a blast furnace to form Fe (s) and CO (g) The balanced reaction for the process is: The substance being oxidized is The substance reduced is In order to make 1510 grams of Fe (s) with 100% yield, one needs to grams of Fe2O3 (s) and use grams of C (s).
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?
3. Pure iron can be prepared from reacting Fe203 with carbon monoxide: Fe2O3 (s) + CO...
3. Pure iron can be prepared from reacting Fe203 with carbon monoxide: Fe2O3 (s) + CO (9) ► Fe (s) + CO2 (g) a. Balance the equation AN Felse
The reaction of iron ore with carbon follows the equation: 2 Fe2O3+ 3 C 4 Fe+3...
The reaction of iron ore with carbon follows the equation: 2 Fe2O3+ 3 C 4 Fe+3 CO2 3. How many grams of Fe can be produced from a mixture of 200 g of Fe2O3 and 300. g of C?
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....
15. (15 points) Iron for the prouction of steel is obtained by a process known as...
15. (15 points) Iron for the prouction of steel is obtained by a process known as smelting, during which iron(III) oxide is reduced by carbon monoxide to yield pure iron: Fe2O3(s) + 3 CO(g) → 2 Fe(s) + 3 CO2(g). a. What is the limiting reagent when 32.55 g Fe2O3(s) and 14.78 g CO(g) are combined? For full credit, clearly show your work.(MW Fe2O3 = 159.69 g/mol; MW CO = 28.01 g/mol) b. How many grams of Fe(s) can be...
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...
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
14. (1 point per blank) Iron ore, Fe2O3 (s), reacts with C (s) in a blast furnace to form Fe (s) and CO (g) The balanced reaction for the process is: The substance being oxidized is The substance reduced is In order to make 1510 grams of Fe (s) with 100% yield, one needs to grams of Fe2O3 (s) and use grams of C (s).
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?
3. Pure iron can be prepared from reacting Fe203 with carbon monoxide: Fe2O3 (s) + CO (9) ► Fe (s) + CO2 (g) a. Balance the equation AN Felse
The reaction of iron ore with carbon follows the equation: 2 Fe2O3+ 3 C 4 Fe+3 CO2 3. How many grams of Fe can be produced from a mixture of 200 g of Fe2O3 and 300. g of C?
15. (15 points) Iron for the prouction of steel is obtained by a process known as smelting, during which iron(III) oxide is reduced by carbon monoxide to yield pure iron: Fe2O3(s) + 3 CO(g) → 2 Fe(s) + 3 CO2(g). a. What is the limiting reagent when 32.55 g Fe2O3(s) and 14.78 g CO(g) are combined? For full credit, clearly show your work.(MW Fe2O3 = 159.69 g/mol; MW CO = 28.01 g/mol) b. How many grams of Fe(s) can be...
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