Final answer:
The incorrect statement pertains to 'activity' under standard conditions for measuring reduction potentials. Standard conditions specify a temperature of 25°C and the standard state generally refers to an activity of 1, accounting for non-ideal behavior of solutions rather than just concentrations of 1 M.
Step-by-step explanation:
The statement that requires correction regarding standard reduction potentials is: "standard conditions for measuring reduction potentials are 25°C and activity". Standard conditions indeed specify a temperature of 25°C (298.15 K), but the term 'activity' referred to here is more complex than simply stating it as 'activity'.
The standard state for measuring reduction potentials is defined with all species in their standard states, which means solution concentrations are 1 M for solutes, pressures are 1 atm for gases, and pure substances are in their pure form (solid or liquid) for other species.
However, when dealing with real solutions, the concept of activity, which takes into account deviations from ideal behavior, is used instead of concentration. In such cases, a standard state corresponds to an activity of 1. This is important for precise quantitative work.
To calculate standard cell potentials and relate them to spontaneity, free energy changes, and equilibrium constants, we use tables of standard reduction potentials and equations that relate these quantities. For example, to determine the spontaneity of a reaction, we would look at the sign of the standard cell potential (ΔE°cell).
A positive value typically indicates a spontaneous reaction under standard conditions, whereas a negative value indicates a nonspontaneous reaction. This potential can also be related to Gibbs free energy (ΔG°) and the equilibrium constant (K), using the equations ΔG° = -nFE°cell and ln K = -ΔG°/(RT), where n is the number of moles of electrons transferred, F is the Faraday constant, R is the gas constant, and T is the temperature in kelvins.