For the equilibrium reaction
`2NO_2(g) hArr N_2O_4(g)` + 60.0 kJ the increase in temperature

Options

A. favours the formation of `N_2O_4`
B. favours the decomposition of `N_2O_4`
C. does not effect the equilibrium
D. stops the reaction.

Explanation

To solve the question regarding the equilibrium reaction \(2NO_2(g) \rightleftharpoons N_2O_4(g) + 60.0 \, \text{kJ}\) and the effect of increasing temperature, we can follow these steps:

### Step-by-Step Solution:

1. **Identify the Reaction and its Enthalpy Change**:
The given reaction is:
\[ 2NO_2(g) \rightleftharpoons N_2O_4(g) + 60.0 \, \text{kJ} \]
Here, the enthalpy change (\( \Delta H \)) is positive, indicating that the reaction is endothermic.

**Hint**: Remember that a positive \( \Delta H \) means heat is absorbed during the reaction.

2. **Apply Le Chatelier's Principle**:
According to Le Chatelier's Principle, if a system at equilibrium is subjected to a change in temperature, the equilibrium will shift in the direction that counteracts that change. Since the reaction is endothermic, increasing the temperature will favor the formation of products.

**Hint**: Think of temperature as a reactant in endothermic reactions; increasing it pushes the equilibrium towards the products.

3. **Determine the Direction of the Shift**:
In this case, increasing the temperature will shift the equilibrium to the right, favoring the formation of \(N_2O_4\).

**Hint**: Visualize the equilibrium as a balance; adding heat (temperature) will tip the balance towards the side that absorbs heat (the products).

4. **Conclusion**:
As a result of the temperature increase, the concentration of \(N_2O_4\) will increase while the concentration of \(NO_2\) will decrease.

**Hint**: The key takeaway is that for endothermic reactions, increasing temperature increases the yield of products.

### Final Answer:
The increase in temperature will lead to an increase in the formation of \(N_2O_4\).