The relationship between equilibrium constant and free energy change is represented as

EmB01

2 years ago

The correct answer is B. δG ° = -RT ln K.

The relationship between the equilibrium constant (K) and the standard free energy change (δG °) is given by the equation:

δG ° = -RT ln K

where:

- δG ° is the standard free energy change (in joules per mole, J/mol)
- R is the gas constant (in joules per mole-kelvin, J/mol·K)
- T is the temperature (in kelvin, K)
- ln is the natural logarithm
- K is the equilibrium constant (unitless)

This equation indicates that a negative δG ° (spontaneous process) corresponds to a large K (favors products), while a positive δG ° (non-spontaneous process) corresponds to a small K (favors reactants).

Chikeziehenry

5 years ago

It is d cus change in ∆G=∆H-∆TS

Dainiel

6 years ago

is the answer not d