For the reaction $N_2 + 3H_2 \rightleftharpoons 2NH_3$,the value of $K_c$ does not depend on: $(a)$ Initial concentration of reactants $(b)$ Pressure $(c)$ Temperature $(d)$ Catalyst

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?

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 $(i)$?

In a chemical reaction,equilibrium is established only when...

In the chemical equilibrium of a reversible reaction,which of the following does not cause any change?

For the equilibrium, $H_{2}O_{(l)} \rightleftharpoons H_{2}O_{(g)},$ which of the following is correct?