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Aug 14, 2020 · Definition of equilibrium constant in terms of forward and reverse rate constants: \[K=\dfrac{k_f}{k_r} \nonumber \] Equilibrium constant expression (law of mass action): \[K=\dfrac{[C]^c[D]^d}{[A]^a[B]^b} \nonumber \]
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Learn about the equilibrium constant (Kc or Kp) of a chemical reaction, which measures the ratio of products to reactants at equilibrium. Find out how to calculate, interpret and apply Kc and Kp, and how they relate to △G, Q and Le Chatelier's principle.
Learn what equilibrium constants are and how to write them for homogeneous and heterogeneous equilibria. Find examples, definitions, and explanations of Kc expressions and values for different reactions.
The equilibrium constant is a dimensionless quantity (has no units). Although the calculation is usually written for two reactants and two products, it works for any numbers of participants in the reaction. Kc in Homogeneous vs. Heterogeneous Equilibrium.
Learn how to define and calculate the equilibrium constant K for reversible reactions, and how to use it to determine the reaction direction and equilibrium concentrations. See graphs, equations and examples of nitrogen dioxide formation and other reactions.
The equilibrium constant of a chemical reaction is the value of its reaction quotient at chemical equilibrium, a state approached by a dynamic chemical system after sufficient time has elapsed at which its composition has no measurable tendency towards further change.
The equilibrium expression links the equilibrium constant, Kc, to the concentrations of reactants and products at equilibrium taking the stoichiometry of the equation into account. So, for a given reaction: aA + bB ⇌ cC + dD. the Kc is defined as follows:
