To determine the correct statement about the given chemical system at dynamic equilibrium at 500 K, let's analyze the properties and characteristics of chemical equilibrium.
The given reaction is:
[tex]\[ 2 N_2O_5(g) \longleftrightarrow 4 NO_2(g) + O_2(g) \][/tex]
At dynamic equilibrium, the following points are true:
1. Dynamic Nature of Equilibrium: At dynamic equilibrium, both the forward and reverse reactions continue to occur. However, they do so at equal rates. This means that there is no net change in the concentrations of the reactants and products over time.
2. Equal Rates: The rates of the forward and reverse reactions are equal at equilibrium. This ensures that the amount of reactants being converted into products is equal to the amount of products being converted back into reactants.
3. Stable Concentrations: As a result of the equal rates, the concentrations of the products and reactants remain constant. The system has reached a state of balance where the amount of each substance does not change with time.
4. No Stopping of Reactions: The forward and reverse reactions do not stop; they continue to occur, but at the same rate, maintaining the dynamic equilibrium.
Given the options:
1. The forward and reverse reactions no longer occur.
2. The rates of the forward and reverse reactions are unequal.
3. The concentrations of the products and reactants do not change.
4. The forward reaction stops at 500 K.
The accurate statement describing the state of the reaction at dynamic equilibrium at 500 K is:
The concentrations of the products and reactants do not change.
Therefore, the correct answer is:
The concentrations of the products and reactants do not change.
