7. Iron is produced from its ore by the reactions: 2C(s) + O2(g) → 2CO(g) Fe2O3...
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....
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?...
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...
Consider the four reactions listed below for the next question. 1. FeO(s)+CO(g)<->Fe(s)+Co2(g) K=0.403 2. 2C(s)+O2(g)<->2CO(g) K=1x10at16 power 3. 2Cl2(g)+2H2O(l)<->4HCl(aq)+O2(g) K=1.9x10 at-15 power 4. C(s)+2H2(g)<->CH4(g) K=27.5 a.Which reaction has the smallest tendency to occur? 1. Reaction a 2. Reaction b 3. Reaction c 4. Reaction d
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?
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
From the enthalpies of reaction 2C(s)+O2(g)→2CO(g)ΔH=−221.0kJ 2C(s)+O2(g)+4H2(g)→2CH3OH(g)ΔH=−402.4kJ calculate ΔH for the reaction CO(g)+2H2(g)→CH3OH(g)
Consider following chemical reactions: 1) CHa(g) +202(8)-CO2(g) 2H20() 2) C(s) O2(g) CO2(g) 3) 2C(s)O2(g) 2CO(g) 4) 3C(s) 2H20()CH4(g)2CO(g) H2O(I) indicates that H2O is in liquid state. If the Enthalpy of reaction for reaction 1, 2, and 3 are -890.4kj, -393.5kj and -221.0kj respectively; try to figure out the Enthalpy of reaction for reaction 4. Please show your work.
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....