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HARI A
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I am familiar with the equation ΔG=ΔG°+RT ln(Q).But I can't derive it.We have to use the equation to derive nernst equation. So please help.
morrobay said:In this reference , post #2 PhaseShifter states: q = Keq
Can someone show how this is ?
Borek said:Do you know what Q is? (To be honest using q is IMHO confusing).
The relationship between Gibbs free energy and equilibrium constant is described by the following equation: ΔG = -RTlnK, where ΔG is the change in Gibbs free energy, R is the gas constant, T is the temperature in Kelvin, and K is the equilibrium constant. This equation shows that the equilibrium constant is directly proportional to the Gibbs free energy change.
Gibbs free energy determines the spontaneity of a chemical reaction. A negative ΔG indicates that the reaction is spontaneous and will proceed in the forward direction. Conversely, a positive ΔG indicates that the reaction is non-spontaneous and will proceed in the reverse direction. When ΔG is equal to zero, the reaction is at equilibrium.
Yes, Gibbs free energy can be used to predict the feasibility of a reaction. A negative ΔG indicates that the reaction is thermodynamically favorable and will occur spontaneously. A positive ΔG indicates that the reaction is thermodynamically unfavorable and will not occur spontaneously. However, the kinetics of a reaction must also be considered in determining its feasibility.
The equilibrium constant is affected by changes in temperature according to the equation lnK2/K1 = -ΔH/R(1/T2 - 1/T1), where K1 and K2 are the equilibrium constants at temperatures T1 and T2 respectively, ΔH is the enthalpy change, and R is the gas constant. This equation shows that the equilibrium constant is inversely proportional to temperature, meaning that an increase in temperature will lead to a decrease in the equilibrium constant.
Yes, the equilibrium constant can be used to calculate the Gibbs free energy change of a reaction using the equation ΔG = -RTlnK. This equation allows us to determine the Gibbs free energy change at any temperature, as long as the equilibrium constant is known. However, it should be noted that the calculated ΔG will only be valid at the temperature for which the equilibrium constant was determined.