Find out the value of `K_(c )` for each of the following equilibrium from the value of `K_(p)`:
a. `2NOCl(g) hArr 2NO(g)+Cl_(2)(g), K_(p)=1.8xx10^(-2)` at `500 K`
b. `CaCO_(3)(s) hArr CaO(s)+CO_(2)(g), K_(p)=167` at `1073 K`

Explanation

To find the value of \( K_c \) from the given \( K_p \) for the reactions, we will use the relationship between \( K_p \) and \( K_c \):

\[ K_p = K_c (RT)^{\Delta N_g} \]

Where:
- \( R \) is the ideal gas constant (0.0831 L·bar/(K·mol))
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