Consider the following reaction
`N_(2)O_(4)(g)hArr2NO_(2)(g)DeltaH=58.6KJ`
What will be the effect of the following changes on the concentration of `N_(2)O_(4)` at equilibrium?
(i) Increasing the pressure (ii) Increasing the temperature
(iii) Increasing the volume
(iv) Adding more `NO_(2)(g)` to the system without changing temperature and pressure (v) Adding catalyst.

Explanation

To analyze the effects of various changes on the concentration of \( N_2O_4 \) at equilibrium for the reaction:

\[ N_2O_4(g) \rightleftharpoons 2NO_2(g) \quad \Delta H = 58.6 \, \text{kJ} \]

we will go through each change step by step.

### Step 1: Increasing the Pressure
- **Analysis**: According to Le Chatelier's principle, if the pressure of a system at equilibrium is increased, the system will shift in the direction that produces fewer moles of gas. In this reaction, we have 1 mole of \( N_2O_4 \) on the reactant side and 2 moles of \( NO_2 \) on the product side. Therefore, increasing the pressure will shift the equilibrium to the left (towards the reactants).
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