Question

consider the reaction.
2so₂(g) + o₂(g)⇌2so₃(g)
when does the given chemical system reach dynamic equilibrium?
○ when the forward and reverse reactions stop
○ when the rate of the forward reaction is higher than the rate of the reverse reaction
○ when the concentration of the reactants is higher than the concentration of the products
○ when the rates of the forward and reverse reactions are equal

Explanation:

Dynamic equilibrium in a chemical reaction is defined as the state where the rate of the forward reaction (conversion of reactants to products) is equal to the rate of the reverse reaction (conversion of products to reactants). At this point, the concentrations of reactants and products remain constant (but the reactions do not stop, so the first option is wrong). If the forward rate is higher, the reaction is still proceeding forward (so second option is wrong). The concentration relationship (reactants vs products) doesn't define equilibrium (equilibrium can have more reactants, more products, or equal amounts depending on the reaction, so third option is wrong). Thus, the correct condition is equal forward and reverse reaction rates.

Answer:

D. when the rates of the forward and reverse reactions are equal (assuming the options are labeled A to D with the last option as D; if original labels were different, adjust accordingly, but based on the options: the correct one is "when the rates of the forward and reverse reactions are equal")