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“K” refers to the equilibrium constant of a chemical reaction. It provides insight into the relationship between the reactants and products when a chemical reaction reaches equilibrium.
The concentration’s equilibrium constant denoted by Kc of a chemical reaction can be defined as the ratio of product’s concentration to reactant’s concentration. Each one raised their respective stoichiometric coefficients.
However, it is essential to be noted that the equilibrium constants are of several types that endow with relationships between reactants and products of equilibrium reactions in terms of different units.
At equilibrium, Forward reaction’s rate = Backward reaction’s rate
i.e. rf= rb
Given a reaction,
aA + bB ⇌ cC + dD
For the above reaction, the equilibrium constant is defined as:
Where Kc, indicates the equilibrium constant that is measured in moles per litre.
The unit of equilibrium constant = [Mole L-1] △n
Where △n= Sum of product’s stoichiometric coefficients – Sum of reactant’s stoichiometric coefficients.
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