What is happening within the system when it is at equilibrium in terms of concentration, reactions that occur, and reaction rates? 2CH4(g) <--> C2H2(g) + 3H2(g)
It is worthy to be mentioned that the equilibrium in this reaction is dynamic equilibrium.
In terms of concentration: the concentration of reactants (CH4) and products (C2H2 & H2) do not change and be constant at the equilibrium, that 2 moles of CH4 give one mole of C2H2 and 3 moles of H2.
In terms of reactions that occur: the reactions that occur at the equilibrium are the forward and the reverse reaction. The forward reaction: 2CH4 → C2H2 + 3H2 and the reverse reaction: C2H2 + 3H2 → 2CH4.
In terms of reaction rates: At equilibrium the rate of the forward reaction is equal to the rate of the reverse reaction.
In a chemical reaction equilibrium is in the state which reacts with both products and reactants. Both reverse and forward are happening and both reaction rates forward and reverse are equal.
