it dependes upon the initial ratio of molar concentration of products to reactants higher the ratio reaction will proceed in the reverse direction and vice versa
Reversible reaction
You think probable to a reversible reaction.
In a reversible reaction, the reactants and products become to a dynamic equilibrium after some time. after gaining this equilibrium, when more reactants are added the equilibrium breaks. So according to the Le Chetelier principle, the reaction will proceed until the equilibrium is gained.
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.
Extent of the reaction measures how far a reaction will proceed before establishing equilibrium state .
Reversible reaction
You think probable to a reversible reaction.
In a reversible reaction, the reactants and products become to a dynamic equilibrium after some time. after gaining this equilibrium, when more reactants are added the equilibrium breaks. So according to the Le Chetelier principle, the reaction will proceed until the equilibrium is gained.
Catalysts can do one or more of the following:enable a chemical reaction to take place,speed up the reaction,allow the reaction to proceed at a lower temperature,change the equilibrium point of a reversible reaction so that more of the desired output is produced.
because i
Under normal circumstances action potential will proceed unilaterally. An action potential cannot proceed down an axon and depolarize in the reverse direction on the same axon. It must carry information on one axon in one direction and then on another axon in a separate direction. In a lab you can depolarize neurons in the middle of an axon and it will depolarize bilaterally.
its called a reversible
It indicates that the reaction can proceed in both directions. It could also mean that the reactions are in a dynamic equilibrium.
When the Gibbs free energy for a reaction is greater than zero, the reaction is "disfavored" - won't proceed in that direction - in fact it may try go in the reverse direction if possible. When the Gibbs free energy for a reaction is less than zero, the reaction is "favored" - it should proceed as written spontaneously. When the Gibbs free energy for a reaction is exactly zero - it is in equilibrium, with the forward and back ward reactions occurring at the same rate.
An exergonic reaction
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.
This is not entirely true.It depends upon the reaction.Some reaction which are reversible can be reversed when suitable force is applied in the opposite direction.Here the force implies Pressure and heat.