[Big-Daddy]

My thermodynamics textbook says that chemical potential can take any of the following symbols: μ (condition-dependent), μ^∇ (standard), μ^Θ (standard) (superscript plimsoll line) and μ^O (standard), with which one of the latter 3 being used depending on the temperature chosen to define standard state.

I have seen that the notation typically used for ΔH under standard conditions of 298.15 K, 1 bar pressure is the ΔH^Θ symbol (and ΔS^Θ similarly). However, ΔG^O is used to denote ΔG under standard conditions of 298.15 K, 1 bar pressure. Should this more correctly be ΔG^Θ (so we write ΔG^Θ=ΔH^Θ-T·ΔS^Θ, so the conditions are the same)? Or perhaps they are all actually ^O?

Also, does ΔG^Θ for a reaction actually refer to the value of ΔG for that reaction under standard conditions of 298.15 K, 1 bar pressure? If so, wouldn't that mean that the equilibrium constant must be 1 under standard conditions (which is not necessarily true), as a result of ΔG=ΔG^Θ+R·T·log_e(Q) and now ΔG=ΔG^Θ under such conditions? If not, what is the actual definition of ΔG^Θ, and with regards to ΔG itself?