Calculate K_p for each reaction. a. N₂O₄(g) ⇌ 2 NO₂(g) K_c = 5.9⨉10^-3 (at 298 K)

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Identify the balanced chemical equation for the reaction: N2O4(g) ⇌ 2NO2(g).

Understand the relationship between Kc and Kp: Kp = Kc(RT)^{\(\Delta\) n}, where R is the gas constant (0.0821 L atm K^{-1} mol^{-1}), T is the temperature in Kelvin, and \(\Delta\) n is the change in moles of gas (moles of products - moles of reactants).

Calculate \(\Delta\) n for the reaction: \(\Delta\) n = 2 - 1 = 1.

Substitute the values into the equation: Kp = (5.9 \(\times\) 10^{-3}) \(\times\) (0.0821 \(\times\) 298)^1.

Simplify the expression to find Kp.

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Equilibrium Constant (Kc and Kp)

The equilibrium constant (Kc) quantifies the ratio of the concentrations of products to reactants at equilibrium for a given reaction at a specific temperature. Kp, on the other hand, is the equilibrium constant expressed in terms of partial pressures of gases. The relationship between Kc and Kp is given by the equation Kp = Kc(RT)^(Δn), where Δn is the change in moles of gas, R is the ideal gas constant, and T is the temperature in Kelvin.

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Kp vs. Kc Formula

Partial Pressure

Partial pressure is the pressure exerted by a single component of a gas mixture. In the context of Kp, it refers to the pressure of each gas in the reaction when it is at equilibrium. The total pressure of the gas mixture is the sum of the partial pressures of all the gases present, and understanding this concept is crucial for calculating Kp from Kc.

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Partial Pressure Calculation

Change in Moles of Gas (Δn)

Δn is defined as the difference between the number of moles of gaseous products and the number of moles of gaseous reactants in a balanced chemical equation. This value is essential for converting Kc to Kp, as it indicates how the number of gas molecules changes during the reaction. A positive Δn suggests an increase in gas moles, while a negative Δn indicates a decrease, affecting the relationship between Kc and Kp.

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