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15. (15 points) Iron for the prouction of steel is obtained by a process known as...
47. Iron (III) oxide reacts with carbon monoxide according to the equation: Fe2O3(s) + 3 CO(g)...
47. Iron (III) oxide reacts with carbon monoxide according to the equation: Fe2O3(s) + 3 CO(g) 2 Fe(s) +3 CO2(8) A reaction mixture initially contains 22.55 g Fe203 and 14.78 g CO. Once the reaction has occurred as completely as possible, what mass (in g) of the excess reactant remains?
Important industrial processes, such as converting iron ore to iron and then to steel, involve coupling...
Important industrial processes, such as converting iron ore to iron and then to steel, involve coupling a non-spontaneous reaction, such as reducing Fe2O3 (iron ore)to metallic iron, with a spontaneous process such as the oxidation of carbon in CO to CO2: Fe2O3 (s) + 3 CO (g) 2 Fe (s) + 3 CO2 (g) Reagent ΔHºf (kJ/mol) ΔSº(J/mol*K) Fe2O3 (s) -824.2 87.4 CO (g) -110.5 197.7 Fe(s) 0 27.3 CO2 (g) -393.5 213.8 Use the thermodynamic data provided above to determine...
5. Under a high-pressure atmosphere of oxygen, the compound C7H11O4NS2 is burned. A. Write the balanced...
5. Under a high-pressure atmosphere of oxygen, the compound C7H11O4NS2 is burned. A. Write the balanced equation for this reaction. You may assume all the nitrogen is converted to NO2 and the sulfur is converted to SO3. Coefficients should represent the smallest whole number ratio of all reactants and products – no fractional coefficients. (7.5 pts.) B. If 77.6 g of the compound is burned, what is the mass of each product? (7.5 pts 6. Consider the reaction: Fe2O3(s) +...
In the thermite reaction, iron (III) oxide is reduced by aluminum to give molten iron, Fe2O3...
In the thermite reaction, iron (III) oxide is reduced by aluminum to give molten iron, Fe2O3 (s) + 2 Al (s) --> 2 Fe (l) + Al2O3 (s) If you begin with 10.0 g of Fe2O3 and 20.0 g Al, Which reactant is limiting? What mass of Fe can be produced? What mass of the excess reactant remains after the limiting reactant is consumed? Set up an amounts table for this problem.
The reduction of iron(III) oxide (Fe203) to pure iron during the first step of steelmaking 2 Fe2O...
The reduction of iron(III) oxide (Fe203) to pure iron during the first step of steelmaking 2 Fe2O3(s) 4 Fe(s) + 3 O2(g) is driven by the high-temperature combustion of coke, a purified form of coal: Cs)+O2(8) CO2(g) alo AG of CO2 and Fe,03 are Suppose at the temperature of a blast furnace the Gibbs free energies of formation Ar 447. kJ/mol and 801. kJ/mol, respectively. Calculate the minimum mass of coke needed to produce 3000. kg of pure iron. Round...
got stuck here урд 5 For Practice 7.8 Recall from Example 7.8 that mining companies extract iron from iron ore accor...
got stuck here
урд 5 For Practice 7.8 Recall from Example 7.8 that mining companies extract iron from iron ore according to the following balanced equation: Fe2O3(s) + 3 CO(g) — >2 Fe(s) + 3 CO2(g) 15979 21.. In a reaction mixture containing 167 g Fe2O3 and 85.8 g CO, CO is the limiting reactant. Calculate the mass of the reactant in excess (which is Fe2O3) that remains after the reaction has gone to completion. Imol Fe2O3 1679 X issing...
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
You must show work in order to receive credit. Make sure to include units and indicate...
You must show work in order to receive credit. Make sure to include units and indicate your final answer by putting a box around your final answer. If you do not box in a response, I will count it as no final answer and you will lose points! 1. Mining companies use this reaction to obtain iron from iron ore: Fe2O3(s) + 3 CO(g) + 2 Fe(s) + 3 CO2(g) The reaction of 167 g Fe2O, with 85.8 g CO...
are these right? im having a hard time on number 2 a-c Experiment 9-Post-lab Questions 1....
are these right? im having a hard time on number 2 a-c
Experiment 9-Post-lab Questions 1. Methanol (CH,OH) can be produced by the reaction o balanced chemical reaction is by the reaction of carbon monoxide (CO) with hydrogen (H). The CO(g) + 2 H (g)-CH2OH) Suppose 14.0 g of carbon monoxide is reacted with 8.0 g of hydrogen 3. Which reactant is the limiting reagent? Carbon monoxide (co) b. What is the theoretical yield for methanol? 16.02 g CH₂OH c....
Iron ore is reduced to pure iron by smelting, during which the iron (III) oxide in...
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...
47. Iron (III) oxide reacts with carbon monoxide according to the equation: Fe2O3(s) + 3 CO(g) 2 Fe(s) +3 CO2(8) A reaction mixture initially contains 22.55 g Fe203 and 14.78 g CO. Once the reaction has occurred as completely as possible, what mass (in g) of the excess reactant remains?
The reduction of iron(III) oxide (Fe203) to pure iron during the first step of steelmaking 2 Fe2O3(s) 4 Fe(s) + 3 O2(g) is driven by the high-temperature combustion of coke, a purified form of coal: Cs)+O2(8) CO2(g) alo AG of CO2 and Fe,03 are Suppose at the temperature of a blast furnace the Gibbs free energies of formation Ar 447. kJ/mol and 801. kJ/mol, respectively. Calculate the minimum mass of coke needed to produce 3000. kg of pure iron. Round...
got stuck here
урд 5 For Practice 7.8 Recall from Example 7.8 that mining companies extract iron from iron ore according to the following balanced equation: Fe2O3(s) + 3 CO(g) — >2 Fe(s) + 3 CO2(g) 15979 21.. In a reaction mixture containing 167 g Fe2O3 and 85.8 g CO, CO is the limiting reactant. Calculate the mass of the reactant in excess (which is Fe2O3) that remains after the reaction has gone to completion. Imol Fe2O3 1679 X issing...
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
You must show work in order to receive credit. Make sure to include units and indicate your final answer by putting a box around your final answer. If you do not box in a response, I will count it as no final answer and you will lose points! 1. Mining companies use this reaction to obtain iron from iron ore: Fe2O3(s) + 3 CO(g) + 2 Fe(s) + 3 CO2(g) The reaction of 167 g Fe2O, with 85.8 g CO...
are these right? im having a hard time on number 2 a-c
Experiment 9-Post-lab Questions 1. Methanol (CH,OH) can be produced by the reaction o balanced chemical reaction is by the reaction of carbon monoxide (CO) with hydrogen (H). The CO(g) + 2 H (g)-CH2OH) Suppose 14.0 g of carbon monoxide is reacted with 8.0 g of hydrogen 3. Which reactant is the limiting reagent? Carbon monoxide (co) b. What is the theoretical yield for methanol? 16.02 g CH₂OH c....
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...
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