Question

2ch4(g) c2h2(g) 3h2(g) describe what is happening within the system when it is at equilibrium in terms of concentrations, reactions that occur, and reaction rates.

Answer 1

Balanced chemical reaction: 2CH₄(g) ⇄ C₂H₂(g) + 3H₂(g).

1) In a chemical reaction, chemical equilibrium is the state in which both reactants (methane CH₄) and products (ethyne C₂H₂ and hydrogen H₂) are present in concentrations which have no further tendency to change with time.  

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

3) Reaction rates of the forward and backward reactions are equal and  there are no changes in the concentrations of the reactants and products.

Answer 2

The balanced reaction that describes the decomposition of methane to produce C2H2 and hydrogen is expressed 2ch4(g) = c2h2(g) + 3h2(g)  In the equilibrium, there are 4 moles of gas products produced from 2 moles of gas reactant. Hence, an increase in volume favors the forward reaction while increase in pressure favors the production of methane (backward). Equilibrium constant is expressed: Kp= (c2H2)^2(H2)^3/(Ch4)^2