Here are the essential concepts you must grasp in order to answer the question correctly.
Gibbs Free Energy (ΔG)
Gibbs Free Energy (ΔG) is a thermodynamic potential that measures the maximum reversible work obtainable from a thermodynamic system at constant temperature and pressure. It is a crucial concept in predicting the spontaneity of a reaction; a negative ΔG indicates a spontaneous process, while a positive ΔG suggests non-spontaneity. The standard Gibbs free energy change (ΔG°) is calculated under standard conditions, typically at 1 atm and 298 K.
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Standard Gibbs Free Energy Change (ΔG°)
The standard Gibbs Free Energy Change (ΔG°) is the change in Gibbs free energy for a reaction when all reactants and products are in their standard states (1 M concentration for solutions, 1 atm pressure for gases) at a specified temperature, usually 298 K. It is derived from the standard enthalpy and entropy changes of the reaction using the equation ΔG° = ΔH° - TΔS°. This value helps in determining the favorability of a reaction under standard conditions.
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Reaction Quotient (Q) and its Relation to ΔG
The reaction quotient (Q) is a measure of the relative amounts of products and reactants present in a reaction at any point in time, calculated using the partial pressures or concentrations of the species involved. It is used to determine the direction in which a reaction will proceed to reach equilibrium. The relationship between ΔG and Q is given by the equation ΔG = ΔG° + RT ln(Q), where R is the gas constant and T is the temperature in Kelvin. This equation allows for the calculation of ΔG under non-standard conditions.
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