Question

How is standard Gibbs energy for a reaction related to equilibrium constant?

Hint:

Use \(\Delta G^\circ = -RT \ln K\) to link thermodynamics with equilibrium.
If \(\Delta G^\circ<0\), then \(K>1\), and the reaction favors products.

Answer 1

Step 1: The standard Gibbs free energy change \(\Delta G^\circ\) is related to the equilibrium constant \(K\) by the formula:
\[\Delta G^\circ = -RT \ln K\]
Step 2: Where:
\(R\) = Universal gas constant = 8.314 J mol\(^{-1}\) K\(^{-1}\)
\(T\) = Temperature in Kelvin
\(K\) = Equilibrium constant of the reaction
Step 3: A negative \(\Delta G^\circ\) implies a spontaneous reaction and a large \(K\).