N2+3H2 <-> 2NH3, The equilibrium constant for the chemical equation is Kp = 0.143 at 225 °C. Calculate the value of the Kc for the reaction at 225 °C.

Kp = Kc(RT)^delta n

where delta n = n products - n reactants.

To calculate the value of Kc for the reaction at 225 °C, we need to use the relationship between Kp and Kc. The equilibrium constant, Kp, is defined as the ratio of the partial pressures of the products to the partial pressures of the reactants, each raised to the power of their respective stoichiometric coefficients.

For the given reaction:
N2 + 3H2 ↔ 2NH3

We can write the expression for Kp as follows:

Kp = (P(NH3))^2 / (P(N2) * P(H2)^3)

To convert Kp to Kc, we need to account for the relationship between partial pressures and concentrations in the ideal gas law. The ideal gas law equation is:

PV = nRT

Where:
P = pressure
V = volume
n = moles of gas
R = ideal gas constant
T = temperature

We can rewrite the equation for Kp in terms of moles:

Kp = (n(NH3))^2 / (n(N2) * n(H2)^3)

Since Kp and Kc are related, we can use the relation:

Kp = Kc * (RT)^Δn

Where:
R = ideal gas constant
T = temperature
Δn = (sum of stoichiometric coefficients of products) - (sum of stoichiometric coefficients of reactants)

In this case, Δn = (2 + 0) - (1 + 3) = -2

Rearranging the equation, we can solve for Kc:

Kc = Kp / (RT)^Δn

Given:
Kp = 0.143
T = 225 °C = 498.15 K
R = 0.0821 L atm/K mol (ideal gas constant)

Substituting the values into the equation, we have:

Kc = 0.143 / (0.0821 * 498.15)^(-2)

Calculating the value, we get:

Kc ≈ 1.83 x 10^4

Therefore, the value of Kc for the reaction at 225 °C is approximately 1.83 x 10^4.