Abstract
The standard free energy change is a function only of temperature. It is independent of pressure and concentration for a specified standard state. Alternative forms of the equilibrium constant can be obtained as one expresses the relationship between activities, and pressures or concentrations. For example, for a gas phase reaction, the standard state one usually chooses is the ideal gas at a pressure of 1 bar. For any given temperature, the [thermodynamic] equilibrium constant is directly related to the standard change in free energy. Since, at any given temperature, the free energy in the standard state for each reactant and product, G°i, is independent of the pressure, it follows that the standard change in free energy for the reaction, ΔrG°, is independent of the pressure. Therefore, at constant temperature, the equilibrium constant K is also independent of the pressure.
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