Certainly! Let's analyze the reaction and the concept of dynamic equilibrium to determine the correct statement:
Consider the chemical reaction:
[tex]\[ 2 \text{N}_2\text{O}_5(g) \longleftrightarrow 4 \text{NO}_2(g) + \text{O}_2(g) \][/tex]
The given condition is that the reaction is at dynamic equilibrium at a temperature of [tex]\( 500 \, \text{K} \)[/tex].
### Dynamic Equilibrium Concept
Dynamic equilibrium occurs in a chemical system when the rates of the forward and reverse reactions are equal, but the reactions continue to occur. Despite these continuous reactions, there is no net change in the concentrations of the reactants and products. This means that while individual molecules are still reacting, the overall concentrations stay constant over time.
Now, let’s evaluate the provided statements given this understanding:
#### 1. The forward and reverse reactions no longer occur.
- This is not correct. Even at equilibrium, both forward and reverse reactions still occur, but at the same rate, so their effects cancel each other out with no net change in the concentrations.
#### 2. The rates of the forward and reverse reactions are unequal.
- This is incorrect. At dynamic equilibrium, the rates of the forward and reverse reactions are equal by definition.
#### 3. The concentrations of the products and reactants do not change.
- This is correct. When a system is at dynamic equilibrium, the concentrations of both the reactants and products remain constant over time.
#### 4. The forward reaction stops at [tex]\(500 \, \text{K}\)[/tex].
- This is incorrect. Both the forward and reverse reactions continue to occur even at equilibrium; they do not stop.
### Conclusion
Given the analysis above, the correct statement that applies to the given chemical system at dynamic equilibrium at [tex]\( 500 \, \text{K} \)[/tex] is:
The concentrations of the products and reactants do not change.
