Question

Consider the following chemical reaction: 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

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.

Answer 2

Answer: It told me

Explanation: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.

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