For the equilibrium
`2NOCl(g) hArr 2NO(g)+Cl_(2)(g)`
the value of the equilibrium constant, `K_(c)` is `3.75 xx 10^(-6)` at `1069 K`. Calcualate the `K_(p)` for the reaction at this temperature?

Explanation

To calculate \( K_p \) for the reaction

\[ 2NOCl(g) \rightleftharpoons 2NO(g) + Cl_2(g) \]

given that the equilibrium constant \( K_c \) is \( 3.75 \times 10^{-6} \) at \( 1069 \, K \), we can follow these steps:

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