Question on: SS3 Chemistry - Chemical Thermodynamics

The relationship between the standard Gibbs free energy change (ΔG°) and the equilibrium constant (K) for a reaction at a given temperature (T) is given by the equation:

ΔG° = -RT ln(K)

where R is the gas constant (8.314 J/(mol·K)) and T is the temperature in Kelvin.

Given ΔG° = -20.0 kJ/mol and T = 298 K, we need to convert ΔG° to J/mol:

ΔG° = -20.0 kJ/mol × 1000 J/1 kJ = -20,000 J/mol

Now, we can calculate the equilibrium constant (K):

K = e(-ΔG° / (RT))

K = e^(-(-20,000 J/mol) / (8.314 J/(mol·K) × 298 K))

K = e^(67.94)

K ≈ 9.42 × 10²⁹

Therefore, the equilibrium constant (K) for the reaction at 298 K is approximately 9.42 × 10²⁹.