Calculate Kc at 303 K for SO2(g) + Cl2(g) ⇌ SO2Cl2(g) if Kp = 34.5 at this temperature.

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Identify the relationship between Kc and Kp using 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.

Determine Δn for the reaction SO2(g) + Cl2(g) ⇌ SO2Cl2(g). Calculate Δn as the difference in moles of gaseous products and reactants: Δn = moles of products - moles of reactants.

Substitute the known values into the equation: Kp = Kc(RT)^(Δn). Use R = 0.0821 L·atm/(mol·K) for the ideal gas constant and T = 303 K.

Rearrange the equation to solve for Kc: Kc = Kp / (RT)^(Δn).

Substitute the values of Kp, R, T, and Δn into the rearranged equation to find Kc.

Key Concepts

Here are the essential concepts you must grasp in order to answer the question correctly.

Equilibrium Constants (Kc and Kp)

Kc and Kp are equilibrium constants that describe the ratio of concentrations or partial pressures of products to reactants at equilibrium. Kc is used for concentrations in mol/L, while Kp is used for partial pressures in atm. The relationship between Kc and Kp is given by the equation Kp = Kc(RT)^(Δn), where Δn is the change in moles of gas during the reaction.

Ideal Gas Law

The Ideal Gas Law (PV = nRT) relates the pressure, volume, temperature, and number of moles of an ideal gas. It is essential for understanding how gases behave under different conditions and is used to derive Kp from Kc. The law assumes that gas particles do not interact and occupy no volume, which is a good approximation under many conditions.

Temperature Dependence of Equilibrium Constants

Equilibrium constants are temperature-dependent, meaning that a change in temperature can alter the values of Kc and Kp. For a given reaction, Kp and Kc can be related through the ideal gas law, but their specific values will vary with temperature. Understanding this relationship is crucial for calculating Kc from Kp when the temperature is specified.

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Magnitude of Equilibrium Constant

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