` K_p` for the reaction
`N_2O_4(g) = 2NO_2(g)`
is 0.66 at `46^@C` . Calculate the per cent dissociation of `N_2O_4` at `46^@C` and a total pressure of 380 mm. What are the partial pressures of `N_2O_4` and `NO_2` at equilibrium?

Explanation

To solve the problem step by step, we will follow the provided information and apply the principles of equilibrium and partial pressures.

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

### Step 2: Define the initial conditions
Let the initial pressure of \( N_2O_4 \) be \( P_0 = 0.5 \, \text{atm} \) (which is equivalent to 380 mmHg). At the start, the pressure of \( NO_2 \) is 0.
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