Iron ore is converted to iron metal in a reaction with carbon.
2 Fe2O3 (s) + 3 C (s) ----------> 4 Fe (s) + 3 CO2 (g)
If 2.24 moles of Fe2O3 are used, what amount of C is needed and what amounts of Fe and CO2, in moles are produced?
_____ mol C
_____ mol Fe
_____ mol CO2
Iron ore is converted to iron metal in a reaction with carbon. 2 Fe2O3 (s) +...
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?
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?
8) Iron ore is reduced to iron with coke (impure carbon). Calculate the mass of Fe that can be produced from Fe2O3 with 15.00 kg of carbon. The reaction may be represented as follows: Fe2O3(s) + 3 C(s) + heat → 2 Fe(l) + 3 CO(g) 9) Given the following reaction: Na2S2O3 + AgBr → NaBr + NasſAg(S203)2] a. How many moles of Na2S2O3 are needed to react completely with 42.7 g of AgBr?! þ. What is the mass of...
Question 1: Iron ore is converted into iron by heating it with coal (carbon) & oxygen: 2Fe2O3(s) + 6C(s) + 3O2(g) → 4Fe(s) + 6CO2(g) What is the molar mass of iron, Fe, in g/mol? Question 2: Iron ore is converted into iron by heating it with coal (carbon) & oxygen: 2Fe2O3(s) + 6C(s) + 3O2(g) → 4Fe(s) + 6CO2(g) Calculate the molar mass of iron(III) oxide in g/mol: Question 3: Iron ore is converted into iron by heating it...
part 1 of 3 Iron is generally produced from iron ore through the reaction Fe2O3(s) + CO(g) −→ Fe(s) + CO2(g) . If 3.3 kg of Fe2O3 are available to react, how much CO is needed? 1. 54.4771 2. 95.8046 3. 105.197 4. 46.9631 5. 20.6637 6. 110.833 7. 61.9912 8. 33.8134 9. 73.2624 10. 65.7483 015 (part 2 of 3) 10.0 points How much Fe can be produced? 1. 53.851 2. 57.608 3. 16.2805 4. 62.6174 5. 72.6362 6....
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...
7. Iron is produced from its ore by the reactions: 2C(s) + O2(g) → 2CO(g) Fe2O3 (s) + 3 CO(g) → Fe(s) + CO2(g) How many moles of O2(g) are needed to produce 4.6 moles of Fe(s)? a. 2.3 b. 3.5 C. 4.6 d. 6.9 e. 13.8
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