Calculate the equilibrium constant for the reaction : `NO(g) + 1/2 O_(2)(g) iff NO_(2)(g)`
Given, `Delta_(f)H^(@) at 298K : NO(g) = 90.4 kJ "mol"^(-1), NO_(2)(g) = 33.8 kJ "mol"^(-1)` and `DeltaS^(@)` at `298 K = -70.8 J K^(-1) "mol"^(-1)`, `R = 8.31 J K^(-1) "mol"^(-1)`.

Explanation

To calculate the equilibrium constant for the reaction:

\[ \text{NO(g)} + \frac{1}{2} \text{O}_2(g) \iff \text{NO}_2(g) \]

we will follow these steps:

### Step 1: Calculate the change in enthalpy (\( \Delta H^\circ \)) for the reaction.

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