The free energy change of the reaction A(g) ⟶B(g) is zero under certain conditions. The standard

step 1 We are given with the reaction from A reactants to B where the value of delta G will be equal to

The free energy change of the reaction A(g) ⟶B(g) is zero...

The free energy change of the reaction $\mathrm{A}(g) \longrightarrow \mathrm{B}(g)$ is zero under certain conditions. The standard free energy change of the reaction is $-42.5 \mathrm{~kJ}$. Which statement must be true about the reaction? a. The concentration of the product is greater than the concentration of the reactant. b. The reaction is at equilibrium. c. The concentration of the reactant is greater than the concentration of the product.

The free energy change of the reaction $\mathrm{A}(g) \longrightarrow \mathrm{B}(g)$ is zero under certain conditions. The standard free energy change of the reaction is $-42.5 \mathrm{~kJ}$. Which statement must be true about the reaction?
a. The concentration of the product is greater than the concentration of the reactant.
b. The reaction is at equilibrium.
c. The concentration of the reactant is greater than the concentration of the product.

Key Concepts

Gibbs Free Energy (?G)

Gibbs free energy represents the maximum reversible work that may be performed by a thermodynamic system at constant temperature and pressure. Its value depends on the actual conditions of the reacting system and is calculated by the relationship ?G = ?G° + RT ln Q, where ?G° is the standard free energy change and Q is the reaction quotient. A ?G value of zero indicates that the system is at equilibrium, meaning no net change in the composition of reactants and products occurs.

Standard Free Energy Change (?G°)

The standard free energy change is the change in free energy when a reaction proceeds under standard state conditions (usually 1 bar pressure for gases and 1 M for solutions). It relates directly to the equilibrium constant by the equation ?G° = -RT ln K, where a negative ?G° implies that the equilibrium lies in favor of the products. This value sets the inherent thermodynamic favorability of the reaction but does not by itself indicate the state of the system under non-standard conditions.

Reaction Quotient (Q)

The reaction quotient, Q, is a measure of the relative amounts of products and reactants present during a reaction at a given point in time. It is calculated similarly to the equilibrium constant but for any set of conditions. In the equation ?G = ?G° + RT ln Q, the value of Q determines how far the reaction is from equilibrium; when Q equals the equilibrium constant (K), ?G becomes zero, signifying that the system is at equilibrium.

Chemical Equilibrium

Chemical equilibrium refers to the state of a reversible reaction where the rate of the forward reaction equals the rate of the reverse reaction, resulting in constant concentrations of all species involved over time. At equilibrium, the free energy change for the reaction (?G) is zero, indicating that the system has reached a state of minimum free energy and no net reaction occurs in either direction. This concept is central to understanding how reaction conditions dictate the distribution of reactants and products.

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