No, a large negative ΔG⦵ indicates spontaneity and the favourability of a reaction in the forward direction, but it doesn't comment on the rate of the reaction. A reaction can be thermodynamically favourable but still proceed very slowly if it has a high energy barrier or activation energy. Reaction kinetics, which deals with reaction rates, and thermodynamics, which addresses the energy changes and direction of reactions, are two different branches. A reaction may be spontaneous due to a negative ΔG⦵ but could be slow due to kinetic constraints.

The value of ΔG⦵ is temperature-dependent. As temperature changes, ΔG⦵ can also change, leading to a shift in the equilibrium position. The relationship between ΔG⦵ and temperature is embedded within the Van't Hoff equation. An increase in temperature can make ΔG⦵ more positive or more negative, depending on the endothermic or exothermic nature of the reaction. As ΔG⦵ and K are related by the equation ΔG⦵ = -RT ln K, a change in ΔG⦵ due to temperature will also lead to a change in K, potentially shifting the position of equilibrium.

Yes, ΔG⦵ can change without altering the concentrations or pressures of reactants and products. While concentrations and pressures play a crucial role in determining the reaction's Gibbs energy under non-standard conditions (ΔG'), ΔG⦵, being the standard Gibbs energy change, is defined for standard conditions. Factors like temperature, as mentioned earlier, can influence ΔG⦵. Changes in the surroundings, including solvents or other conditions that affect the inherent energy states of reactants and products, can also impact ΔG⦵ without altering their concentrations or pressures.

The value of ΔG under non-standard conditions, often represented as ΔG', takes into account the actual concentrations or pressures of reactants and products at any given moment, not just at equilibrium. The relationship is given by ΔG' = ΔG⦵ + RT ln Q, where Q is the reaction quotient. Depending on whether Q is greater or lesser than K, ΔG' can be positive or negative, respectively. If ΔG' is negative, the system will shift towards products, and if positive, it will shift towards reactants. Hence, non-standard conditions can shift the equilibrium position by influencing the value of ΔG'.

At equilibrium, there is no net change in the concentrations of reactants or products. The rates of the forward and reverse reactions are equal, which means there's no driving force pushing the reaction in one direction or the other. When there's no tendency for the reaction to favour the products or reactants, the potential for the system to do work is nullified. As ΔG represents the maximum work the system can do, a ΔG value of zero at equilibrium indicates the system cannot perform any more work in terms of driving the reaction in either direction.