`K_(p)` for the reaction `N_(2) O_(4) (g) rarr 2NO_(2)(g)` is 0.66 at `46^(@)C`. Calculate the percent dissociation of `N_(2)O_(4)` at `46^(@)C` and a total pressue of 0.5 atm. Also calculate the partial pressure of `N_(2)O_(4)` and `NO_(2)` at equilibrium.

Explanation

To solve the problem, we need to calculate the percent dissociation of \( N_2O_4 \) at \( 46^\circ C \) and a total pressure of \( 0.5 \, \text{atm} \). We will also find the partial pressures of \( N_2O_4 \) and \( NO_2 \) at equilibrium.

### Step 1: Write the balanced chemical equation
The balanced chemical equation for the reaction is:
\[ N_2O_4(g) \rightleftharpoons 2NO_2(g) \]

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