Mark the correct statement in a reversible reaction.

For the equilibrium system $H_2 + I_2 \rightleftharpoons 2HI$,if the concentration of the reactants is increased at $25\,^oC$,what happens to the value of $K_c$?

For a reversible reaction involving two reactants,if the concentration of the reactants is doubled,the equilibrium constant will:

One mole of $A_{(g)}$ is heated to $200^{\circ} C$ in a one litre closed flask,until the following equilibrium is reached:
$A_{(g)} \rightleftharpoons B_{(g)}$
The rate of forward reaction at equilibrium is $0.02 \ mol \ L^{-1} \ min^{-1}$. What is the rate (in $mol \ L^{-1} \ min^{-1}$) of the backward reaction at equilibrium?

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

When chemical equilibrium is established in a reaction...