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14.3: Homogeneous Equilibria for Gaseous Reactions
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Homogeneous Equilibria for Gaseous Reactions
 
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14.3: Homogeneous Equilibria for Gaseous Reactions

Homogeneous Equilibria for Gaseous Reactions

For gas-phase reactions, the equilibrium constant may be expressed in terms of either the molar concentrations (Kc) or partial pressures (Kp) of the reactants and products. A relation between these two K values may be simply derived from the ideal gas equation and the definition of molarity. According to the ideal gas equation:

Eq1

Molar concentration or molarity is given by number of moles divided by the volume:

Eq2

Thus,

Eq3

where P is partial pressure, V is volume, n is number of moles, R is the gas constant, T is temperature, and M is molar concentration.

For the gas-phase reaction: m A + n B ⇌ x C + y D

Eq4

And so, the relationship between Kc and KP is

Eq5

where Δn is the difference in the molar amounts of product and reactant gases, in this case:

Eq6

This text has been adapted from Openstax, Chemistry 2e, Section 13.2 Equilibrium Constants.

Tags

Homogeneous Equilibria Gaseous Reactions Equilibrium Constant Partial Pressures Molar Concentrations Reversible Reaction Stoichiometric Coefficients Kp Kc Ideal Gas Equation Molarity Individual Partial Pressures Molar Concentration Equivalent Modified Expression

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