What is Gibbs free energy and why is it significant in predicting the spontaneity of chemical reactions?

Calculate the change in Gibbs free energy for a reaction at equilibrium using the equation ΔG = ΔH - TΔS, given ΔH = 0 kJ/mol, T = 298 K, and ΔS = 0 J/mol·K.

If the reaction quotient (Q) is greater than the equilibrium constant (K), in which direction will the reaction proceed?

Analyze how physiological conditions differ from standard conditions and their impact on Gibbs free energy calculations.

Given ΔH = -100 kJ/mol, T = 298 K, and ΔS = -0.2 kJ/mol·K, calculate ΔG and interpret its implications for the reaction's spontaneity.

For a reaction with K = 0.5 at 298 K, calculate ΔG° using the equation ΔG° = -RTlnK.

Calculate the actual change in Gibbs free energy for a reaction under physiological conditions with ΔG° = -20 kJ/mol, R = 8.315 J/mol·K, T = 310 K, and Q = 0.05 using the equation ΔG = ΔG° + RTlnQ.