kc kp equilibrium calculations
Overview
This lesson explores equilibrium constants, Kc and Kp, which quantify the relative amounts of reactants and products at equilibrium for reversible reactions. We will learn how to write expressions for these constants, perform calculations involving them, and understand their relationship to reaction conditions.
Introduction to Equilibrium Constants (Kc)
For a general reversible reaction: **aA + bB ⇌ cC + dD** The equilibrium constant, **Kc**, is defined as: **Kc = ([C]^c [D]^d) / ([A]^a [B]^b)** Where: * **[A], [B], [C], [D]** represent the equilibrium molar concentrations (in mol dm⁻³) of reactants and products. * **a, b, c, d** are the s...
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Key Concepts
- Chemical Equilibrium: A state where the rate of the forward reaction equals the rate of the reverse reaction, and the concentrations of reactants and products remain constant.
- Equilibrium Constant (Kc): A value that expresses the ratio of product concentrations to reactant concentrations at equilibrium, each raised to the power of their stoichiometric coefficients.
- Equilibrium Constant (Kp): A value that expresses the ratio of partial pressures of gaseous products to gaseous reactants at equilibrium, each raised to the power of their stoichiometric coefficients.
- Homogeneous Equilibrium: An equilibrium where all reactants and products are in the same physical state (e.g., all gases or all aqueous solutions).
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Exam Tips
- →Always write down the balanced chemical equation and the Kc/Kp expression before starting calculations. This earns method marks.
- →Pay close attention to units! Ensure concentrations are in mol dm⁻³ for Kc and partial pressures are consistent (e.g., all Pa or all atm) for Kp. Remember to convert temperature to Kelvin for Kp = Kc(RT)^Δn.
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