the rate of the forward reaction is greater than the rate of the reverse reaction.
When a reaction has reached equilibrium, the rate of the forward reaction is equal to the rate of the reverse reaction. At equilibrium, the concentrations of reactants and products remain constant over time, but the reaction is still ongoing.
All motion ceases
If you continuously add reactants even after the reaction has attained the equilibrium then according to Le Chatelier's principle, the reaction will again proceed in forward direction in order to neutralise the reactants and once again the attain the state of equilibrium.
The equilibrium constant can tell us how the reaction is going. If the constant is grater than one there are more products than reactants, so the reaction os closer to completion. If the equilibrium constant is less than 1 it shows that there are a lot more products than reactants so the reaction has not really started yet.
Something is in "equilibrium" when it is in a state of perfect balance or rest. All forces acting on it are equal and opposite. It is in a "minimum" energy state.
When a reaction has reached equilibrium, the rate of the forward reaction is equal to the rate of the reverse reaction. At equilibrium, the concentrations of reactants and products remain constant over time, but the reaction is still ongoing.
All motion ceases
All motion ceases
In a chemical reaction, equilibrium does not favor the weaker acid. Equilibrium is reached when the rates of the forward and reverse reactions are equal, regardless of the strength of the acids involved.
The value of the equilibrium constant indicates the extent to which a reaction has reached equilibrium. A high value means that the equilibrium strongly favors the products, while a low value means the equilibrium strongly favors the reactants.
Not necessarily. The equilibrium constant (K) quantifies the extent of a reaction at equilibrium, but it does not directly correlate to the rate of reaction. A large equilibrium constant indicates that the reaction favors the products at equilibrium, but the rate of the reaction depends on factors such as concentration, temperature, and catalysts.
An increase in temperature can generally speed up the time it takes for equilibrium to be reached in a chemical reaction. This is because higher temperatures provide more energy to the reactant molecules, increasing their kinetic energy and collision frequency, which in turn accelerates the rate of the reaction towards equilibrium.
It tells whether products or reactants are favored at equilibrium
In an organic chemical reaction, it is said to be in equilibrium , when the forward reaction is equal to the backward reaction. Here is an example. Ethanoic Acid and Ethanol are in equilibrium with water and ethyl ethanoate CH3COOH + CH3CH2OH H2O + CH3CH2-O-C(=O)CH3
If you continuously add reactants even after the reaction has attained the equilibrium then according to Le Chatelier's principle, the reaction will again proceed in forward direction in order to neutralise the reactants and once again the attain the state of equilibrium.
An equilibrium occurs when the rate of the forward reaction equals the rate of the reverse reaction. This means that the concentrations of reactants and products remain constant over time. Equilibrium can only be reached in a closed system under certain conditions, such as constant temperature and pressure.
Dynamic equilibrium is reached when the rate of the forward reaction equals the rate of the reverse reaction in a closed system. This means that the concentrations of reactants and products remain constant over time. The system appears to be at rest even though the reactions are still ongoing.