Chemical equilibrium is the result of
when the reaction attains equal mass of products and reactants
stoppage of further reaction
loss of pressure in the system
both the foward and reverse reactions attaining equal rates.
all of the reactants being converted into products
The correct answer and explanation is :
The correct answer is “both the forward and reverse reactions attaining equal rates.”
Explanation:
Chemical equilibrium occurs in a reversible reaction when the rates of the forward and reverse reactions become equal, meaning that the concentration of reactants and products remains constant over time. At equilibrium, the system does not stop reacting; rather, the reactions continue to occur, but because they happen at the same rate in both directions, there is no net change in the concentrations of reactants and products.
Let’s break it down:
- Forward reaction: Reactants are converted into products.
- Reverse reaction: Products are converted back into reactants.
- At equilibrium, the rate at which reactants are converted into products equals the rate at which products are converted back into reactants. Therefore, the concentrations of both reactants and products remain constant, even though both reactions are still occurring.
It’s important to note that equilibrium does not imply that the amounts of reactants and products are equal. The relative amounts depend on the equilibrium constant (K) and the nature of the reaction.
Now, let’s address the other options:
- When the reaction attains equal mass of products and reactants: This is not necessarily true at equilibrium. The concentrations of products and reactants are not necessarily equal at equilibrium. They are dependent on the reaction’s equilibrium constant.
- Stoppage of further reaction: At equilibrium, reactions do not stop; they continue at equal rates.
- Loss of pressure in the system: While pressure changes can affect the equilibrium position, it does not describe the definition of equilibrium itself.
In conclusion, chemical equilibrium is defined by the point at which the forward and reverse reactions occur at the same rate, ensuring the concentrations of reactants and products remain constant over time.
Here is a graphical representation of chemical equilibrium. The two reversible reactions are shown, with both forward and reverse reactions occurring at equal rates, leading to constant concentrations of reactants and products at equilibrium.