Home › JEE Main › Thermodynamics & Kinetic Theory › The relationship between $\Delta G^\circ$ and th…
The relationship between $\Delta G^\circ$ and the equilibrium constant $K$ for a chemical reaction is:
A$\Delta G^\circ = -R T K$
B$\Delta G^\circ = R T / \ln K$
C$\Delta G^\circ = -R T \ln K$
D$\Delta G^\circ = R T \ln K$
Answer & Solution
Correct answer: C. $\Delta G^\circ = -R T \ln K$
At equilibrium $\Delta G = 0 = \Delta G^\circ + R T \ln Q$ with $Q = K$, so $\Delta G^\circ = -R T \ln K$. A negative $\Delta G^\circ$ corresponds to $K > 1$ (product-favoured equilibrium); a positive $\Delta G^\circ$ to $K < 1$ (reactant-favoured); $\Delta G^\circ = 0$ to $K = 1$.
Related questions
A reaction has $\Delta H = -100$ kJ and $\Delta S = +200$ J/K. At $T = 298$ K, $\Delta G$ Among solid ice, liquid water, and water vapour at the same temperature, entropy is:Hess's law states that the standard enthalpy change for a reaction:For a reaction occurring at constant pressure in an open beaker, the heat absorbed equals:There are two spherical balls $A$ and $B$ of the same material with same surface, but the A cylindrical rod with one end in a steam chamber and the other end in ice results in meltAn ideal gas expands isothermally from a volume $V_{1}$ to $V_{2}$ and then compressed to Two cylinders $A$ and $B$ fitted with pistons contain equal amounts of an ideal diatomic g