For a reversible system at a constant temperature, the value of `K_(c)` increases if the concentrations are changed at equilibrium.

With increase in temperature, the value of equilibrium constant

For a reversible reaction at constant temperature and at constant pressure the equilibrium composition of reaction mixture corresponds to the lowest point on Gibbls energy Vs progress of reaction diagrams as shown. At equilibrium Gibbs energy of reaction is equal to zero. The value of "log"_(10) K_(eq) is equal to [ k_(eq) is the equilibrium coustant]

In a reversible reaction, two substances are in equilibrium. If the concentration of each one is reduced to half, the equilibrium constant will be

In an equilibrium A+B hArr C+D , A and B are mixed in vessel at temperature T. The initial concentration of A was twice the initial concentration of B. After the equilibrium has reaches, concentration of C was thrice the equilibrium concentration of B. Calculate K_(c) .

Assertion : K_(p) = K_(c) for all reaction. Reason : At constant temperature, the pressure of the gas is proportional to its concentration.

It the absolute temperature of sun increased by 2% then the value solar constant will change by