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14.3: Equilibria for Gaseous Reactions and Heterogeneous Reactions
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Equilibria for Gaseous Reactions and Heterogeneous Reactions
 
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14.3: Equilibria for Gaseous Reactions and Heterogeneous 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.

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