Does a reaction cease when it reaches dynamic equilibrium?
No, it doesn't.
In actuality, the rate at which reactants react to form products (the forward reaction) is equal to the rate at which products form reactants (the backward reaction) at dynamic equilibrium.
Actually, the definition of dynamic refers to a reaction that never stops, and the definition of equilibrium refers to a forward reaction that proceeds at the same rate as the reverse reaction.
It differs from static equilibrium, which denotes the point at which the reaction has stopped (perhaps analogous to a reaction's endpoint, but that's just my opinion...).
Plus Fact: The reaction is still occurring at dynamic equilibrium; it just looks to have stopped because there are no outward signs of it.
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No, a reaction does not cease when it reaches dynamic equilibrium. At dynamic equilibrium, the rates of the forward and reverse reactions are equal, but the reaction continues to occur in both directions.
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When evaluating a one-sided limit, you need to be careful when a quantity is approaching zero since its sign is different depending on which way it is approaching zero from. Let us look at some examples.
When evaluating a one-sided limit, you need to be careful when a quantity is approaching zero since its sign is different depending on which way it is approaching zero from. Let us look at some examples.
When evaluating a one-sided limit, you need to be careful when a quantity is approaching zero since its sign is different depending on which way it is approaching zero from. Let us look at some examples.
When evaluating a one-sided limit, you need to be careful when a quantity is approaching zero since its sign is different depending on which way it is approaching zero from. Let us look at some examples.
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- Which of the next salts have better solubility in 1.0M NH3 than in distilled water? Na2CO3, KCl, AgBr, KNO3

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