The term equilibrium is used in the context of reversible reactions that reach a point where concentrations no longer change. The term steady-state is used in enzyme kinetics when the concentration of the enzyme-substrate complex no longer changes (or hardly changes, in case of a quasi steady state). It is also used to describe multi-step biochemical pathways. Is there a difference between the two, given that both concern a situation where concentrations don't change over time?

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    $\begingroup$ From a (simplified) biochemistry perspective when an organism reaches equilibrium that means it died. Organisms strive for steady state consumption of energy to stay alive. $\endgroup$
    – A.K.
    Commented Mar 11, 2019 at 15:57
  • $\begingroup$ In an equilibrium forward and reverse rates are equal; in a steady state the reverse reaction is overwhelmed by an increased forward reaction and a secondary reaction that competes with the reverse reaction. This requires an energy flux that increases the entropy of the system. When that energy flux falters the system trends towards equilibrium. That is why it gets cold at night and you die when you stop eating. It can get complicated; consider Global Warming or all the steps one must take to stay alive. $\endgroup$
    – jimchmst
    Commented May 21 at 15:56

2 Answers 2


Yes, equilibrium and steady-state are distinct concepts.

A reaction is at equilibrium if reactants and products are both present, the forward and reverse rates are equal and the concentrations don't change over time. If this is the only reaction in a closed, isolated system, the entropy in the system is constant.

Steady-state implies a system that is not at equilibrium (entropy increases). A species is said to be at steady state when the rate of reactions (or more general, processes) that form the species is equal to the rate of reactions (or processes) that remove the species.

In both cases, there are rates ($\mathrm{rate}_1$ and $\mathrm{rate}_2$) that are equal. For an equilibrium, the forward and reverse rate of the same reaction are equal to each other. For a steady state, the rates of processes leading to increase of the concentration of a species are equal to the rates of processes leading to decrease of the concentration of the same species.

$$\ce{A <=>[rate_1][rate_2] B}\ \ \ \ \ vs \ \ \ \ \ \ce{source->[rate_1]C->[rate_2]sink} $$

For an equilibrium, all concentrations are constant over time. For a steady-state, there is a net reaction, so some amounts change (the amount of source and sink), while at least one species - the one at steady state - has a constant concentration as long as the conditions of steady state prevail.

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    $\begingroup$ @KarstenTheis: In a closed system, where the source equal the sink, does the steady-state mean the same thing as equilibrium? $\endgroup$ Commented Dec 20, 2019 at 9:03
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    $\begingroup$ @TheLastCipher I think of steady-state as non-equilibrium. It is possible that some folks define steady-state such that equilibrium is a special case of steady state. Certainly, if the source equals the sink, the system will attain equilibrium eventually. $\endgroup$
    – Karsten
    Commented Dec 20, 2019 at 14:53

In short, equilibrium is a static process characterized by an equilibrium constant and does not have a time component. Steady state is a kinetic process characterized by rate constants and determined by the half-life of the substance with respect to the process. Time is an important dimension here. An example of a steady state process is seen in the formation of an enzyme-substrate complex as described so nicely by Karsten Theis in the post above. Another example is the administration of a drug to a person. The drug is continuously absorbed into the systemic circulation, continuously be distributed to the target site(s), continuously be metabolized and continuously be removed by excretion out of the body. These processes are collectively known as the 4 pharmacokinetic parameters.

  • $\begingroup$ Equilibrium is not static. $\endgroup$
    – jimchmst
    Commented May 21 at 19:44

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