In the reaction of nitrogen and hydrogen how is ammonia produced even though the reaction is reversible?
Because the forward and reverse reactions are occurring at the same rates, ammonia is produced.
Concentration determines the rate of reaction, so when the reactant concentration is high, the forward reaction will start out fast and slow down as it drops.
The reverse reaction will likewise begin slowly and then pick up speed based on the same logic. Until the forward and reverse reaction rates equalize, these two processes will persist.
We now declare that equilibrium has been reached in the reaction, as demonstrated by:
The reason it is called "dynamic" is that while all species concentrations stay constant, both forward and reverse reactions are occurring simultaneously.
According to Mukhtar's response, the Haber Process prevents the system from ever reaching equilibrium because it is a continuous process.
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Ammonia is produced in the reaction between nitrogen and hydrogen because the reaction is favored in the forward direction under certain conditions, such as high pressure and a catalyst. This drives the equilibrium towards the formation of ammonia, despite the reaction being reversible.
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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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