Equilibrium Expression
The equilibrium expression for the given reaction is:

K_c = [NO]²[Cl₂]/[NOCl]²

where [NO], [Cl₂], and [NOCl] represent the molar concentrations of NO, Cl₂, and NOCl, respectively.

Conversion from K_c to K_p
To calculate the value of K_p at 1069 K, we need to convert the equilibrium constant K_c into K_p using the following equation:

K_p = K_c * (RT)^Δn

where R is the ideal gas constant (0.0821 L·atm/(K·mol)), T is the temperature in Kelvin (1069 K), and Δn is the change in the number of moles of gas.

Calculating Δn
In the given reaction, the number of moles of gas on the product side is 2 (2 moles of NO) + 1 (1 mole of Cl₂) = 3 moles. The number of moles of gas on the reactant side is 2 (2 moles of NOCl). Therefore, Δn = 3 - 2 = 1.

Calculating K_p
Using the equation K_p = K_c * (RT)^Δn, we can calculate K_p as follows:

K_p = 3.75 × 10^-6 * (0.0821 L·atm/(K·mol) * 1069 K)¹

Simplifying the equation:

K_p = 3.75 × 10^-6 * (88.9649 L·atm/(mol·K))

K_p ≈ 3.34 × 10^-4 atm

Explanation
The equilibrium constant K_c is a measure of the concentrations of the reactants and products at equilibrium. It is defined as the ratio of the product concentrations to the reactant concentrations, with each concentration raised to the power of its stoichiometric coefficient.

To calculate the equilibrium constant K_p, we need to convert K_c using the equation K_p = K_c * (RT)^Δn. The value of K_p will depend on the temperature and the change in the number of moles of gas (Δn) between the reactants and products.

In this case, the value of K_p at 1069 K is approximately 3.34 × 10^-4 atm. This means that at equilibrium, the concentration of the products