Thank you for visiting Consider the following reaction at equilibrium What effect will increasing the temperature have on the system tex text Fe 3 text O 4 s text. This page is designed to guide you through key points and clear explanations related to the topic at hand. We aim to make your learning experience smooth, insightful, and informative. Dive in and discover the answers you're looking for!
Answer :
Sure! Let's break down the problem and understand the concept involved step-by-step.
### Understanding the Reaction and Temperature Effect:
1. Reaction and ΔH° Value:
- We have a chemical reaction:
[tex]\[ \text{Fe}_3\text{O}_4(s) + \text{CO}(g) \rightleftharpoons 3 \text{FeO}(s) + \text{CO}_2(g) \][/tex]
- The change in enthalpy (ΔH°) for this reaction is given as +35.9 kJ.
2. Interpreting ΔH°:
- A positive ΔH° (+35.9 kJ) indicates that the reaction absorbs heat. This means the reaction is endothermic.
3. Effect of Temperature on Equilibrium:
- According to Le Chatelier's Principle, if a system at equilibrium is subjected to a change (like a change in temperature), the system will adjust to counteract that change and restore a new equilibrium.
- For an endothermic reaction, heat is considered as a reactant.
4. Increasing Temperature:
- When the temperature is increased, you effectively add "heat" to the system.
- For an endothermic reaction, adding heat will cause the equilibrium to shift in the direction where heat is absorbed as a way to counter this addition.
5. Direction of Equilibrium Shift:
- Therefore, increasing the temperature will shift the equilibrium to the right, toward the formation of more products (3 FeO and COâ‚‚).
### Conclusion:
- By increasing the temperature, we are favoring the forward reaction because it requires (absorbs) heat. This means more products will be formed.
Thus, the final answer is: The reaction will shift to the right in the direction of products.
### Understanding the Reaction and Temperature Effect:
1. Reaction and ΔH° Value:
- We have a chemical reaction:
[tex]\[ \text{Fe}_3\text{O}_4(s) + \text{CO}(g) \rightleftharpoons 3 \text{FeO}(s) + \text{CO}_2(g) \][/tex]
- The change in enthalpy (ΔH°) for this reaction is given as +35.9 kJ.
2. Interpreting ΔH°:
- A positive ΔH° (+35.9 kJ) indicates that the reaction absorbs heat. This means the reaction is endothermic.
3. Effect of Temperature on Equilibrium:
- According to Le Chatelier's Principle, if a system at equilibrium is subjected to a change (like a change in temperature), the system will adjust to counteract that change and restore a new equilibrium.
- For an endothermic reaction, heat is considered as a reactant.
4. Increasing Temperature:
- When the temperature is increased, you effectively add "heat" to the system.
- For an endothermic reaction, adding heat will cause the equilibrium to shift in the direction where heat is absorbed as a way to counter this addition.
5. Direction of Equilibrium Shift:
- Therefore, increasing the temperature will shift the equilibrium to the right, toward the formation of more products (3 FeO and COâ‚‚).
### Conclusion:
- By increasing the temperature, we are favoring the forward reaction because it requires (absorbs) heat. This means more products will be formed.
Thus, the final answer is: The reaction will shift to the right in the direction of products.
Thank you for reading the article Consider the following reaction at equilibrium What effect will increasing the temperature have on the system tex text Fe 3 text O 4 s text. We hope the information provided is useful and helps you understand this topic better. Feel free to explore more helpful content on our website!
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Rewritten by : Jeany
