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The following reaction occurs in the Blast Furnace where iron ore is reduced to iron metal:
Fe2O3(s)+3 CO(g) ⇌ 2 Fe(l)+3 CO2(g)
Using the Le Chatelier’s principle, predict which one of the following will not disturb the equilibrium?
Fe2O3(s)+3 CO(g) ⇌ 2 Fe(l)+3 CO2(g)
Using the Le Chatelier’s principle, predict which one of the following will not disturb the equilibrium?
- a)Removal of CO
- b)Removal of CO2
- c)Addition of CO2
- d)Addition of Fe2O3
Correct answer is option 'D'. Can you explain this answer?
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The following reaction occurs in the Blast Furnace where iron ore is r...
Principle, explain how the reaction can be shifted to favor the production of iron metal.
According to Le Chatelier's principle, if a stress is applied to a system in equilibrium, the system will respond by shifting in a direction that minimizes the effect of the stress. In the case of the reaction in the blast furnace, the stress can be applied by manipulating the concentration of the reactants or products, the temperature, or the pressure.
To favor the production of iron metal, we can increase the concentration of CO gas. According to Le Chatelier's principle, an increase in the concentration of a reactant will shift the equilibrium towards the products. In this case, increasing the concentration of CO gas will shift the equilibrium towards the formation of iron metal.
Another way to favor the production of iron metal is by decreasing the concentration of CO2 gas. Again, according to Le Chatelier's principle, a decrease in the concentration of a product will shift the equilibrium towards the products. In this case, decreasing the concentration of CO2 gas will shift the equilibrium towards the formation of iron metal.
Additionally, increasing the temperature can favor the production of iron metal. According to Le Chatelier's principle, an increase in temperature will shift the equilibrium in the endothermic direction. In this case, the formation of iron metal is an endothermic reaction, so increasing the temperature will shift the equilibrium towards the formation of iron metal.
Finally, increasing the pressure can also favor the production of iron metal. According to Le Chatelier's principle, an increase in pressure will shift the equilibrium towards the side with fewer moles of gas. In this case, the formation of iron metal has fewer moles of gas compared to the reactants, so increasing the pressure will shift the equilibrium towards the formation of iron metal.
In summary, to favor the production of iron metal in the blast furnace, we can increase the concentration of CO gas, decrease the concentration of CO2 gas, increase the temperature, or increase the pressure.
According to Le Chatelier's principle, if a stress is applied to a system in equilibrium, the system will respond by shifting in a direction that minimizes the effect of the stress. In the case of the reaction in the blast furnace, the stress can be applied by manipulating the concentration of the reactants or products, the temperature, or the pressure.
To favor the production of iron metal, we can increase the concentration of CO gas. According to Le Chatelier's principle, an increase in the concentration of a reactant will shift the equilibrium towards the products. In this case, increasing the concentration of CO gas will shift the equilibrium towards the formation of iron metal.
Another way to favor the production of iron metal is by decreasing the concentration of CO2 gas. Again, according to Le Chatelier's principle, a decrease in the concentration of a product will shift the equilibrium towards the products. In this case, decreasing the concentration of CO2 gas will shift the equilibrium towards the formation of iron metal.
Additionally, increasing the temperature can favor the production of iron metal. According to Le Chatelier's principle, an increase in temperature will shift the equilibrium in the endothermic direction. In this case, the formation of iron metal is an endothermic reaction, so increasing the temperature will shift the equilibrium towards the formation of iron metal.
Finally, increasing the pressure can also favor the production of iron metal. According to Le Chatelier's principle, an increase in pressure will shift the equilibrium towards the side with fewer moles of gas. In this case, the formation of iron metal has fewer moles of gas compared to the reactants, so increasing the pressure will shift the equilibrium towards the formation of iron metal.
In summary, to favor the production of iron metal in the blast furnace, we can increase the concentration of CO gas, decrease the concentration of CO2 gas, increase the temperature, or increase the pressure.
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The following reaction occurs in the Blast Furnace where iron ore is reduced to iron metal:Fe2O3(s)+3 CO(g) 2 Fe(l)+3 CO2(g)Using the Le Chatelier’s principle, predict which one of the following will not disturb the equilibrium?a)Removal of COb)Removal of CO2c)Addition of CO2d)Addition of Fe2O3Correct answer is option 'D'. Can you explain this answer?
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The following reaction occurs in the Blast Furnace where iron ore is reduced to iron metal:Fe2O3(s)+3 CO(g) 2 Fe(l)+3 CO2(g)Using the Le Chatelier’s principle, predict which one of the following will not disturb the equilibrium?a)Removal of COb)Removal of CO2c)Addition of CO2d)Addition of Fe2O3Correct answer is option 'D'. Can you explain this answer? for JEE 2025 is part of JEE preparation. The Question and answers have been prepared according to the JEE exam syllabus. Information about The following reaction occurs in the Blast Furnace where iron ore is reduced to iron metal:Fe2O3(s)+3 CO(g) 2 Fe(l)+3 CO2(g)Using the Le Chatelier’s principle, predict which one of the following will not disturb the equilibrium?a)Removal of COb)Removal of CO2c)Addition of CO2d)Addition of Fe2O3Correct answer is option 'D'. Can you explain this answer? covers all topics & solutions for JEE 2025 Exam. Find important definitions, questions, meanings, examples, exercises and tests below for The following reaction occurs in the Blast Furnace where iron ore is reduced to iron metal:Fe2O3(s)+3 CO(g) 2 Fe(l)+3 CO2(g)Using the Le Chatelier’s principle, predict which one of the following will not disturb the equilibrium?a)Removal of COb)Removal of CO2c)Addition of CO2d)Addition of Fe2O3Correct answer is option 'D'. Can you explain this answer?.
The following reaction occurs in the Blast Furnace where iron ore is reduced to iron metal:Fe2O3(s)+3 CO(g) 2 Fe(l)+3 CO2(g)Using the Le Chatelier’s principle, predict which one of the following will not disturb the equilibrium?a)Removal of COb)Removal of CO2c)Addition of CO2d)Addition of Fe2O3Correct answer is option 'D'. Can you explain this answer? for JEE 2025 is part of JEE preparation. The Question and answers have been prepared according to the JEE exam syllabus. Information about The following reaction occurs in the Blast Furnace where iron ore is reduced to iron metal:Fe2O3(s)+3 CO(g) 2 Fe(l)+3 CO2(g)Using the Le Chatelier’s principle, predict which one of the following will not disturb the equilibrium?a)Removal of COb)Removal of CO2c)Addition of CO2d)Addition of Fe2O3Correct answer is option 'D'. Can you explain this answer? covers all topics & solutions for JEE 2025 Exam. Find important definitions, questions, meanings, examples, exercises and tests below for The following reaction occurs in the Blast Furnace where iron ore is reduced to iron metal:Fe2O3(s)+3 CO(g) 2 Fe(l)+3 CO2(g)Using the Le Chatelier’s principle, predict which one of the following will not disturb the equilibrium?a)Removal of COb)Removal of CO2c)Addition of CO2d)Addition of Fe2O3Correct answer is option 'D'. Can you explain this answer?.
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