In which of the following reactions,the concentration of product is higher than the concentration of reactant at equilibrium? $(K = \text{equilibrium constant})$

For the equilibrium $A \rightleftharpoons B$,the variation of the rate of the forward $(a)$ and reverse $(b)$ reaction with time is given by:

For the reaction $H_2O_{(s)} \rightleftharpoons H_2O_{(l)}$ at $0\,^\circ C$ and normal pressure:

For the reaction $A + B \rightleftharpoons C + D$,the equilibrium constant is $K$. If the initial moles of $A$ and $B$ are $1.0 \ mol$ each,what will be the value of the equilibrium constant in a second experiment under the same conditions if the initial moles of $A$ and $B$ are $2 \ mol$ and $3 \ mol$ respectively?

The equilibrium constant in a reversible reaction at a given temperature:

Which of the following statements is correct regarding the equilibrium constant $(K)$?