At dynamic equilibrium the reaction on both sides occur at the same rate and the mass on both sides of the equilibrium does not undergo any change. This condition can be achieved only when the value of \(\Delta G\) is (a) \(-1\) (b) \(+1\) (c) \(+2\) (d) 0

Short Answer

Expert verified
\(\Delta G\) must be zero (d) at dynamic equilibrium because it indicates that there is no net energy change driving the reaction in either direction.

Step by step solution

01

Understanding Dynamic Equilibrium

Dynamic equilibrium is a state of a reversible reaction where the rate of the forward reaction is equal to the rate of the backward reaction, resulting in no net change in the concentrations of the reactants and products over time.
02

Relation of \(\Delta G\) with Equilibrium

The Gibbs free energy change (\(\Delta G\)) for a reaction at equilibrium is zero because there is no net change in the system. If \(\Delta G\) were positive or negative, the system would not be at equilibrium as the reaction would favor the formation of either products or reactants, respectively.

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Key Concepts

These are the key concepts you need to understand to accurately answer the question.

Gibbs Free Energy (G)
Gibbs free energy, denoted as G, plays a crucial role in understanding chemical reactions and predicting the direction in which they proceed. It's a thermodynamic quantity representing the maximum amount of work that a system can perform at constant temperature and pressure when it is closed to matter transfer. When G is negative, it indicates that a reaction can spontaneously proceed in the forward direction; conversely, a positive G suggests that the reaction is non-spontaneous and may proceed in the reverse direction.

At dynamic equilibrium, the G of the reaction equals zero (G = 0). This is because there is no net change in the system; the reaction proceeds equally in both the forward and reverse directions. Thus, no additional work can be extracted, and the system is thermodynamically stable. Understanding G is essential for predicting how a reaction will behave under certain conditions, and for manipulating processes to make them more efficient.
Reversible Reactions
Reversible reactions are chemical reactions that can proceed in both the forward and reverse directions. This means the products can react to form the original reactants and vice versa. The ability to move in both directions is fundamental to reaching an equilibrium state.

These reactions are characterized by the chemical equilibrium that can be reached when the forward and reverse reaction rates are equal. Unlike irreversible reactions, reversible reactions do not go to completion and reactants are always present with products. This concept is pivotal in various fields, from industrial synthesis to biochemical reactions within living organisms. Reversible reactions are often represented by a double arrow (rightleftharpoons) in chemical equations to denote the two-way process.
Equilibrium State
An equilibrium state in chemistry is the point at which the rates of the forward and reverse reactions in a reversible reaction are equal, and the concentrations of the reactants and products remain constant over time. It's important to note that even though the macroscopic properties remain constant, reactions at the molecular level are still occurring — it's a dynamic state rather than a static one.

This concept is often misunderstood because the term 'equilibrium' suggests a lack of change. However, equilibrium refers to a balance of changes, with no net effect on the overall system. At equilibrium, predictable by the equilibrium constant (K), reactions have reached a state where the system's Gibbs free energy is at its minimum, and no external work is being done. Therefore, the answer to the exercise is (d) 0, as this indicates that Delta G is zero, a hallmark of dynamic equilibrium.
Chemical Kinetics
Chemical kinetics is the study of the rates of chemical processes and the factors that affect these rates. It involves understanding how various variables such as temperature, pressure, concentration, and the presence of catalysts can influence how quickly a reaction proceeds toward equilibrium or completion.

In the context of dynamic equilibrium, kinetics is crucial because it determines how fast the reaction approaches equilibrium. Depending on the kinetics of the forward and reverse reactions, a system might reach equilibrium quickly or slowly. Therefore, when studying a system at dynamic equilibrium, one is looking at a 'snapshot' where the kinetic rates of the forward and reverse reactions are matched perfectly, even though the individual molecules are in constant motion and continuous conversion from reactants to products and back again.

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