If the concentration of reactants is increased by $x$ times,the equilibrium constant $K$ will become ................

Explain chemical equilibrium with an example of a chemical reaction.

For the equilibrium process $H_2O_{(\ell)} \rightleftharpoons H_2O_{(g)}$ at $1 \, \text{atm}$ and $373 \, K$,which of the following is true?

In a reversible reaction $A \overset{k_1}{\underset{k_2}{\longleftrightarrow}} B$,the initial concentrations of $A$ and $B$ are $a$ and $b$,and the equilibrium concentrations are $(a - x)$ and $(b + x)$ respectively. Express $x$ in terms of $k_1, k_2, a$,and $b$.

If the equilibrium constant of a reaction is $K_c = 1.6 \times 10^{12}$,then at equilibrium,the system will contain:

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