Chemical Equilibrium Constants: Kp Calculation

Understanding Chemical Equilibrium Constants: Kc and Kp

Chemical equilibrium is a state in a reaction where the rates of the forward and reverse reactions are equal. At equilibrium, the concentrations of reactants and products remain constant. Equilibrium constants, such as Kc and Kp, are used to quantify the extent of a chemical reaction at equilibrium.

Kc is the equilibrium constant expressed in terms of molar concentrations of reactants and products. It is calculated using the formula Kc = [products] / [reactants].

Kp, on the other hand, is the equilibrium constant expressed in terms of partial pressures of gas-phase reactants and products. It is calculated using the formula Kp = (Pproducts)^m / (Preactants)^n, where m and n are the coefficients of the products and reactants in the balanced chemical equation.

For a given equilibrium reaction, the values of Kc and Kp are related by the equation Kp = Kc(RT)^(Δn), where R is the gas constant, T is the temperature in Kelvin, and Δn is the difference in the total moles of gaseous products and reactants.

Given that the Kc value for the equilibrium reaction is 407 at 23.4 °C, the value of Kp is also 407. The temperature of the reaction does not affect the values of Kc and Kp, as they are independent of temperature.

In conclusion, the value of Kp for the equilibrium reaction with a Kc of 407 at 23.4 °C is 407, indicating the equilibrium partial pressures of the gases in the reaction.