Answer
Increasing the temperature causes more NO₂ to form and less N₂O₄.
Solution
To predict how increasing the temperature affects the equilibrium of the reaction:
\[ 2 \mathrm{NO}_{2} \rightleftarrows \mathrm{N}_{2}\mathrm{O}_{4} + \text{heat} \]
we can apply **Le Chatelier's Principle**. This principle states that if a dynamic equilibrium is disturbed by changing the conditions, the position of equilibrium will shift to counteract the change.
### **Understanding the Reaction:**
- **Exothermic Reaction:** The forward reaction (formation of \(\mathrm{N}_{2}\mathrm{O}_{4}\)) releases heat, indicating it's exothermic.
- **Heat as a Product:** Since heat is a product, the reaction can be viewed as:
\[ 2 \mathrm{NO}_{2} \rightleftarrows \mathrm{N}_{2}\mathrm{O}_{4} + \text{heat} \]
### **Effect of Increasing Temperature:**
- **Adding Heat:** Increasing the temperature effectively adds heat to the system.
- **Le Chatelier's Response:** To counteract the added heat, the equilibrium will shift in the direction that **absorbs heat**. In this case, the **reverse reaction** (decomposition of \(\mathrm{N}_{2}\mathrm{O}_{4}\)) is endothermic and absorbs heat.
### **Resulting Shift:**
- **Shift Toward Reactants:** The equilibrium will shift to the **left**, favoring the formation of more \(\mathrm{NO}_{2}\) and reducing the concentration of \(\mathrm{N}_{2}\mathrm{O}_{4}\).
### **Summary:**
- **Increase in Temperature → Equilibrium Shifts Left → More \(\mathrm{NO}_{2}\), Less \(\mathrm{N}_{2}\mathrm{O}_{4}\)**
This shift helps absorb the added heat, thereby minimizing the effect of the temperature increase on the system.
**Diagrammatic Representation:**
\[
\begin{align*}
\text{Before Temperature Increase:} & \quad \mathrm{2NO}_{2} \rightleftarrows \mathrm{N}_{2}\mathrm{O}_{4} + \text{heat} \\
\text{After Temperature Increase:} & \quad \leftarrow \quad \text{Shift to the left} \quad \rightarrow
\end{align*}
\]
**Conclusion:**
Increasing the temperature favors the endothermic direction (the reverse reaction), resulting in an increase in \(\mathrm{NO}_{2}\) and a decrease in \(\mathrm{N}_{2}\mathrm{O}_{4}\).
**Reference:**
- Le Chatelier's Principle: Understanding how changes in concentration, temperature, and pressure affect chemical equilibria.
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**Note:** Always consider the nature of the reaction (exothermic or endothermic) when applying Le Chatelier's Principle to predict shifts in equilibrium.
**Answer:**
Increasing the temperature adds heat to the system. Since the forward reaction is exothermic (produces heat), adding heat shifts the equilibrium to the left, favoring reactants. Thus, higher temperature causes more NO₂ to form and less N₂O₄.
Reviewed and approved by the UpStudy tutoring team
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