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 CO₂).
### 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 CO₂).
### 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.
