The concentration quotient of a reversible reaction is Q, and the equilibrium constant is K. What do youconclude if (i) `Q=K(ii) Q gt K(iii) Q lt K `?

For a hypothetical reaction 4A+5B hArr 4P +6Q . The equilibrium constant K_(c ) has units.

In a reversible reaction, if the concentration of reactants are doubles, the equilibrium constant K will:

Assertion : If reaction quotient, Q_(c) for a particular reaction is greater than K_(c) the reaction will proceed in the direction of reactants. Reason : Reaction quotient is defined in the same way as the equilibrium constant K_(c) except that the concentrations in Q_(c) are not necessarily equilibrium values.

Assertion:- The reaction quotient Q, has the same presentation form as the equilibrium constant K and Q is evaluated using any given concentrations of the species involved in the reaction, and not necesssarily equilibrium concenetrations. Reason:- If the numerical value of Q is not the same as the value of equilibrium constant, that time reaction will never proceed.

Assertion: The reaction quotient, Q has the same form as the equilibrium constant K_(eq) , and is evaluated using any given concentrations of the species involved in the reaction, and not necessarily equilibrium constrations. Reason: If the numerical value of Q is not the same as the value of equilibrium constant, a reaction will occur.

The Nernst equation E= E^(@) -RT/nF in Q indicates that the Q will be equal to equilibrium constant K_c when: