Chemical equilibrium is dynamic in nature because

Given the reactions at $500 \ K$:
$(i) \ H_{2(g)} + 1/2 O_{2(g)} \rightleftharpoons H_2O_{(g)}$,$K_c = 2.4 \times 10^{47}$
$(ii) \ H_2O_{(g)} \rightleftharpoons H_{2(g)} + 1/2 O_{2(g)}$,$K_c = 4.1 \times 10^{-48}$
What does the magnitude of $K_c$ indicate about the formation of the product in reaction $(i)$?

For the process $H_2O_{(s)} \rightleftharpoons H_2O_{(l)}$ at $0^{\circ}C$ and $1 \ atm$ pressure,which of the following is true?

Which statement for the equilibrium constant is true for the reaction $A + B \rightleftharpoons C$?

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?