What is the relationship between the free-energy change under nonstandard-state conditions, ∆G, the free-energy change under standard-state conditions, ∆G°, and the reaction quotient, Q?

Verified step by step guidance

1. Step 1: Understand the concept of free energy change (∆G) in a chemical reaction, which indicates the spontaneity of the reaction. A negative ∆G means the reaction is spontaneous, while a positive ∆G means it is non-spontaneous.
2. Step 2: Recognize that ∆G° is the free energy change under standard-state conditions, which are typically 1 atm pressure for gases, 1 M concentration for solutions, and pure solids or liquids for other phases at a specified temperature (usually 298 K).
3. Step 3: Learn about the reaction quotient, Q, which is a measure of the relative amounts of products and reactants present during a reaction at a given point in time. It is calculated using the same expression as the equilibrium constant, K, but for non-equilibrium conditions.
4. Step 4: Use the relationship between ∆G, ∆G°, and Q, which is given by the equation: ∆G = ∆G° + RT ln(Q), where R is the universal gas constant (8.314 J/mol·K) and T is the temperature in Kelvin.
5. Step 5: Analyze how this equation shows that the free energy change under nonstandard conditions (∆G) depends on both the standard free energy change (∆G°) and the reaction quotient (Q). When Q = 1, ∆G = ∆G°. When Q < K, ∆G is negative, indicating the reaction will proceed forward. When Q > K, ∆G is positive, indicating the reaction will proceed in reverse.