Question

Equilibrium of a chemical reaction as viewed by kinetics is in a:

• A. Static steady state
• B. Dynamic steady state
• C. Dynamic unsteady state
• D. Static unsteady state

Hint:

Chemical equilibrium is not static — it's dynamic with equal rates in both directions. Thus, it's a \textbf{dynamic steady state}.

Answer 1

The Correct Option is B

Step 1: Understanding Chemical Equilibrium from a Kinetics Viewpoint
From a kinetic perspective, chemical equilibrium does not mean that the reactants and products stop reacting. Instead, it means that the rates of the forward and reverse reactions are equal, so the concentrations of the species remain constant over time. Step 2: Dynamic vs Static
- Dynamic: Because both forward and reverse reactions are continuously occurring.
- Static: Would imply no molecular activity — incorrect for equilibrium. Step 3: Steady State vs Unsteady State
- Steady state: The macroscopic properties (concentration, pressure, etc.) remain constant with time.
- Unsteady state: Variables change over time. Conclusion: Since equilibrium involves ongoing (dynamic) molecular activity while the overall system properties remain constant (steady), it is a dynamic steady state.