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 \( K_c \) for the given equilibria from the values of \( K_p \), we can use the relationship between \( K_p \) and \( K_c \):

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

Where:
- \( R \) is the gas constant (0.0831 L·bar/K·mol or 0.0821 L·atm/K·mol)
...