Pace-iit & Medical

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The relationship between the equilibrium constants \(K_{p}\) (partial pressures) and \(K_{c}\) (molar concentrations) for a gaseous reaction is given by the equation \(K_{p}=K_{c}(RT)^{\Delta n}\), where \(R\) is the ideal gas constant, \(T\) is the absolute temperature in Kelvin, and \(\Delta n\) is the change in the number of moles of gas (moles of gaseous products - moles of gaseous reactants). This formula connects the two constants, showing how \(K_{p}\) varies with \(K_{c}\) based on temperature and the stoichiometry of the gas. Formula Breakdown: \(K_{p}\): Equilibrium constant in terms of partial pressures of gases.\(K_{c}\): Equilibrium constant in terms of molar concentrations (molarity) of gases.R: Ideal gas constant (e.g., 0.0821 L·atm/mol·K or 8.314 J/mol·K, depending on units).T: Absolute temperature in Kelvin (K).\(\Delta n\): Change in moles of gas = (total moles of gaseous products) - (total moles of gaseous reactants).

Kp and Kc are equilibrium constants for gas-phase reactions, with Kp using partial pressures and Kc using molar concentrations, linked by the formula Kp = Kc(RT)^Δn, where R is the gas constant, T is temperature (Kelvin), and Δn is the change in moles of gas (products minus reactants). When Δn=0, Kp=Kc; when Δn>0, Kp>Kc; and when Δn