Answer
(a) $$K_c = \frac{[CO]^2[O_2]}{[CO_2]^2}$$
$$K_p = \frac{P_{CO}^2}{P_{O_2}P_{CO_2}^2}$$
(b) $$K_c = \frac{[O_3]^2}{[O_2]^3}$$
$$K_p = \frac{P_{O_3}^2}{P_{O_2}^3}$$
(c) $$K_c = \frac{[COCl_2]}{[CO][Cl_2]}$$
$$K_p = \frac{P_{COCl_2}}{P_{CO}P_{Cl_2}}$$
(d) $$K_c = \frac{[CO][H_2]}{[H_2O]}$$
$$K_p = \frac{P_{CO}P_{H_2}}{P_{H_2O}}$$
(e) $$K_c = \frac{[H^+][HCOO^-]}{[HCOOH]}$$
(f) $$K_c = [O_2]$$
$$K_p = P_{O_2}$$
Work Step by Step
The $K_p$ expression follows this pattern:
$$K_p = \frac{P_{products}}{P_{reactants}}$$
Where the exponent of each partial pressure is equal to the balance coefficient of the compound.
The $K_c$ expression is very similar, but it uses the concentration of the compounds, and every compound that is not in the form of a pure solid or a pure liquid appear on the expression.
If there is not any compound in the gaseous form, the $K_p$ is not applicable.
