Answered

IDNLearn.com offers a unique blend of expert answers and community insights. Receive prompt and accurate responses to your questions from our community of knowledgeable professionals ready to assist you at any time.

Consider the following chemical reaction:

[tex]\[2 \, CH_4(g) \leftrightarrow C_2H_2(g) + 3 \, H_2(g)\][/tex]

Describe what is happening within the system when it is at equilibrium in terms of concentrations, reactions that occur, and reaction rates.

Sagot :

GinnyAnsweridn
When the system is at equilibrium for the given chemical reaction:
[tex]\[ 2 \text{CH}_4(g) \leftrightarrow \text{C}_2\text{H}_2(g) + 3 \text{H}_2(g) \][/tex]

several important aspects must be considered:

### Concentrations:
1. Concentration Constancy: The concentrations of the reactants ([tex]\(\text{CH}_4\)[/tex]) and the products ([tex]\(\text{C}_2\text{H}_2\)[/tex] and [tex]\(\text{H}_2\)[/tex]) remain constant over time. This means that the amounts of [tex]\(\text{CH}_4\)[/tex], [tex]\(\text{C}_2\text{H}_2\)[/tex], and [tex]\(\text{H}_2\)[/tex] in the system do not change as the system is at equilibrium.

### Reactions Occurring:
2. Forward Reaction: The reaction where 2 methane molecules ([tex]\(2 \text{CH}_4\)[/tex]) are converted into one acetylene molecule ([tex]\(\text{C}_2\text{H}_2\)[/tex]) and three hydrogen molecules ([tex]\(3 \text{H}_2\)[/tex]):
[tex]\[ 2 \text{CH}_4 \rightarrow \text{C}_2\text{H}_2 + 3 \text{H}_2 \][/tex]

3. Backward Reaction: Simultaneously, the reverse reaction also occurs where one acetylene molecule ([tex]\(\text{C}_2\text{H}_2\)[/tex]) and three hydrogen molecules ([tex]\(3 \text{H}_2\)[/tex]) are converted back into two methane molecules ([tex]\(2 \text{CH}_4\)[/tex]):
[tex]\[ \text{C}_2\text{H}_2 + 3 \text{H}_2 \rightarrow 2 \text{CH}_4 \][/tex]

### Reaction Rates:
4. Equal Rates: At equilibrium, the rate of the forward reaction (conversion of [tex]\(\text{CH}_4\)[/tex] to [tex]\(\text{C}_2\text{H}_2\)[/tex] and [tex]\(\text{H}_2\)[/tex]) is equal to the rate of the backward reaction (conversion of [tex]\(\text{C}_2\text{H}_2\)[/tex] and [tex]\(\text{H}_2\)[/tex] back to [tex]\(\text{CH}_4\)[/tex]). This balance ensures that there is no net change in the concentrations of the reactants or products over time.

In summary, at equilibrium, the concentrations of methane ([tex]\(\text{CH}_4\)[/tex]), acetylene ([tex]\(\text{C}_2\text{H}_2\)[/tex]), and hydrogen ([tex]\(\text{H}_2\)[/tex]) remain constant. Both the forward and backward reactions are occurring simultaneously with equal rates, ensuring that the system remains in a state of dynamic equilibrium.
Thank you for being part of this discussion. Keep exploring, asking questions, and sharing your insights with the community. Together, we can find the best solutions. Discover insightful answers at IDNLearn.com. We appreciate your visit and look forward to assisting you again.