Dynamic equilibrium

A reversible chemical reaction is one that may continue in both forward (left to right) and backward (right to left) directions. When the forward and reverse reaction rates are equal, the reactant and product species concentrations stay constant throughout time, and the system is in equilibrium. To illustrate the reversible nature of the reaction, a distinctive double arrow is employed. In equilibrium systems, the relative concentrations of reactants and products vary widely; some systems include predominantly products at equilibrium, while others contain mostly reactants, and still others have significant amounts of both.

What is Dynamic equilibrium?

Only reversible reactions reach dynamic equilibrium, which happens when the forward reaction rate equals the reverse reaction rate. The forward and reverse reactions are still occurring in these equations, but the two rates are equal and constant, thus they’re also at equilibrium.

Changing a reaction’s temperature, pressure, or concentration can cause the equation’s equilibrium to move and knock it out of dynamic equilibrium. 

This is why, after leaving a Coke can open for a long period, it will finally turn “flat,” with no more bubbles. This is due to the fact that the soda can is no longer a closed system, allowing the carbon dioxide to interact with the environment. This throws it out of dynamic equilibrium, causing the gaseous form of carbon dioxide to escape until no more bubbles remain. 

Examples of dynamic equilibrium

If a reaction is reversible and the forward and reverse speeds are equal, it will be in dynamic equilibrium. Assume you’re making a solution that’s saturated with an aqueous solution of NaCl. If you then add solid NaCl crystals to the solution, the NaCl will dissolve and recrystallize at the same time. When the rate of dissolution of the NaCl equals the rate of recrystallization, the reaction:

NaCl(s) ⇌ Na+(aq) + Cl-(aq),will be in dynamic equilibrium.

NO2 (g) + CO(g) = NO(g) + CO2 (g) (again, as long as the two rates are equal). 

Nitrogen dioxide (NO2) interacts with carbon monoxide (CO) to produce nitrogen oxide (NO) and carbon dioxide (CO2), while nitrogen oxide and carbon dioxide react to produce nitrogen dioxide and carbon monoxide in the opposite process.

If you can detect variations in the quantity of reactants or products while watching a process, you know it’s not in dynamic equilibrium. (Just because you can’t see any changes doesn’t mean it’s in dynamic equilibrium; it may be in static equilibrium or the changes are too tiny to see with the human eye.

4 Fe(s) + 6 H2O(l) + 3O2 (g) = 4 Fe(OH)3 is an example of an equation that could never be in dynamic equilibrium (s). 

This is the equation for rust formation. Because the response arrow only travels one way (which is why a rusted automobile won’t get shiny again on its own), we can see that it’ll never be in dynamic equilibrium.

Dynamic equilibrium meaning

The word “equilibrium” comes from the Latin word “equilibrium,” which literally means “an equal balance.” As a result, we may define it as a condition in which opposing forces are balanced or a system that does not change over time, i.e. there is no net force acting.

There are two forms of equilibrium: static equilibrium and dynamic equilibrium. 

A static equilibrium is a body condition in which the resulting force exerted on an object is zero and the object is immobile.

Chemistry’s idea of dynamic equilibrium is crucial. It’s crucial to comprehend how anything may be both active and balanced at the same time.

What is the difference between dynamic equilibrium and static equilibrium?

Though you look at reactions in dynamic equilibrium and static equilibrium, neither will show any apparent changes, and it will appear as if nothing is happening. 

Static equilibrium reactions, on the other hand, are substantially different from dynamic equilibrium reactions.

When a process reaches static equilibrium (also known as mechanical equilibrium), there is no movement between the reactants and products. Both the forward and reverse reaction rates are zero, indicating that the reaction is complete.

While reactions in dynamic equilibrium are reversible (meaning they may go either way), reactions in static equilibrium are irreversible (meaning they can only go one way). 

Both dynamic and static equilibrium, on the other hand, are instances of systems in steady state, where the net force effect on the systems is zero.

Conclusion

When the forward and reverse reaction rates are equal, the reactant and product species concentrations stay constant throughout time, and the system is in equilibrium. If a reaction is reversible and the forward and reverse speeds are equal, it will be in dynamic equilibrium. If you can detect variations in the quantity of reactants or products while watching a process, you know it’s not in dynamic equilibrium. A static equilibrium is a body condition in which the resulting force exerted on an object is zero and the object is immobile. Both dynamic and static equilibrium, on the other hand, are instances of systems in steady state, where the net force effect on the systems is zero.