Consider the following chemical reaction: describe what is happening within the system when it is at equilibrium in terms of concentrations, reactions that occur, and reaction rates.

When we study a chemical reaction in state of equilibrium it is said to be in chemical equilibrium

There are two types of equilibrium

a) static

b) dynamic

In case of dynamic equilibrium, the two reverse process do occur but with same speed

Its like filling a bucket filled bucket which has a hole in it

It appears that bucket is filled always however there is regular inflow and outflow of water in it

In chemical reactions

The rate of forward reaction is equal to rate of backward reaction

A <===>B

So here rate of formation of A is equal to rate of formation of B when system is at equilibrium

so net there is no change in the concentration of either reactant (A) or product (B)

However there is continuous formation and decomposition of both A and B

The equilibrium in the system is a dynamic equilibrium.

At equilibrium, the rate of the forward reaction (CH4 decomposing into C2H2 and H2) is equal to the rate of the reverse reaction (C2H2 and H2 reacting to form CH4).

At equilibrium, the concentrations of all substances are not changing.

At equilibrium, both the forward and reverse reactions are still occurring.

Explanation:

word for word on edge

56 moles of   lieter in chemistry