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The reaction of iron ore with carbon follows the equation: 2 Fe2O3+ 3 C 4 Fe+3...
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...
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?
The reaction of iron ore with carbon follows the equation: 2Fe2O3 + 3C + 3C02 → 4Fe In a reaction, 500 g of Fe2O3 are mixed with 100 g of C. The actual yield of Fe is 5.0 g, what is the percent yield of iron? o 40% 0 60% 20% O 80 % 10 %
1. Consider the following reaction: Fe2O3(s) + 3 COA) 2 Fe(s) + 3 CO29) a. Using dimensional analysis, calculate how many grams of carbon dioxide, CO2, (44.0g/mol) should be produced from 15.97g of Fe,0, (159.7g/mol) reacting with 230.0 g of CO in the following reaction? (6 pts) b. Which is the limiting reactant? (4 points) c. If the % yield of this reaction was 10% how many grams of CO2 would be produced? (4 pts) 2. Balance the following chemical...
1. Consider the following reaction: Fe2O3(s) + 3 COA) 2 Fe(s) + 3 CO29) a. Using dimensional analysis, calculate how many grams of carbon dioxide, CO2, (44.0g/mol) should be produced from 15.97g of Fe,0, (159.7g/mol) reacting with 230.0 g of CO in the following reaction? (6 pts) b. Which is the limiting reactant? (4 points) c. If the % yield of this reaction was 10% how many grams of CO2 would be produced? (4 pts) 2. Balance the following chemical...
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(III) oxide reacts with carbon to give iron and carbon monoxide. Fe2O3(s)+3C(s)→2Fe(s)+3CO(g) How many grams of C are required to react with 29.0 g of Fe2O3? How many grams of CO are produced when 41.0 g of C reacts? How many grams of Fe can be produced when 6.20 g of Fe2O3 reacts?
1. To get iron out of iron ore (the stuff that actually comes out of the ground), you need to heat it with charcoal (C). The reaction is: 2(Fe2O3) + C .......... 4 Fe + 3 (CO2) How many kilograms of iron would you produce by processing 15.00 kg of iron ore? 2. Burning octene is: C8H16 + 12 (O2) ......... 8 (CO2) + 8 (H2O) How many grams of O2 would you require to burn 2.00 moles of octene?...
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
To get iron out of iron ore (the stuff that actually comes out of the ground), you need to heat it with charcoal (C). The reaction is: 2(Fe2O3) + 3C .......... 4 Fe + 3 (CO2) How many moles of carbon would you need to process 2.37 moles of iron ore?