Answer:
Equation is: 2CH4(g) <----> C2H2(g) + 3H2(g)
Explanation:
In the reaction above;
1.) 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). This is because it is a reversible reaction.
2.) At equilibrium, the concentrations of all substances are not changing.
3.) At equilibrium, both the forward and reverse reactions are still occurring.
But if the pressure of the system is increased, the equilibrium position will shift to the left according to le Chatelier's principle since there are fewer number of moles of gaseous atoms at the left.
At equilibrium, the rate of the reactant (methane) and the products (ethyne and hydrogen gas) will be the same since the reaction is a reversible reaction.
The chemical reaction is given as:
2CH₄ (g) ↔ C₂H₂(g) + 3H₂(g)
In terms of concentration at equilibrium, the components of the chemical reaction will evolve and change in the way that gets it closer to its equilibrium. Hence, when the equilibrium is reached, there will be no additional changes provided the system stays undisturbed.
Finally, if any factor affects the equilibrium may be in terms of the addition of reactants or increase in pressure, the system will tend to move in the direction that its effect will be countered.
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