In the equilibrium, $H_{2} + I_{2} \rightleftharpoons 2 HI$, if at a given temperature the concentrations of the reactants are increased, the value of the equilibrium constant, $K_{C}$, will

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 $b$.

Explain chemical equilibrium with an example of a chemical reaction.

The $K_c$ for $H_{2(g)} + I_{2(g)} \rightleftharpoons 2HI_{(g)}$ is $64$. If the volume of the container is reduced to one-half of its original volume,the value of the equilibrium constant will be

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

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