For the reaction $N_2 + 3H_2 \rightleftharpoons 2NH_3$,the equilibrium constant is $K$. What will be the equilibrium constant for the reaction $NH_3 \rightleftharpoons \frac{1}{2}N_2 + \frac{3}{2}H_2$?

The equilibrium constant for the reaction $SO_{3(g)} \rightleftharpoons SO_{2(g)} + \frac{1}{2} O_{2(g)}$ is $K_c = 4.9 \times 10^{-2}$. The value of $K_c$ for the reaction $2SO_{2(g)} + O_{2(g)} \rightleftharpoons 2SO_{3(g)}$ will be

Given below are certain reactions. Identify the reaction for which $K_p = K_c$.

Find the value of $\frac{P}{K_p}$ for the reaction at a certain temperature: $2NOBr_{(g)} \rightleftharpoons 2NO_{(g)} + Br_{2(g)}$,where $P$ is the total pressure of gases at equilibrium and $P_{Br_2} = \frac{P}{9}$.

In the reaction,$A_{(s)} + B_{(g)} \rightleftharpoons 2C_{(s)} + 2D_{(g)}$,equilibrium is established. If the pressure of $B$ is doubled,then to reestablish the equilibrium,how many times does the pressure of $D$ become as compared to its initial pressure?

$2X_{6(g)} \rightleftharpoons 4X_{3(g)}$
$A$ $20 \ L$ box contains $X_6$ and $X_3$ at equilibrium at $1500 \ K$. The equilibrium constant $K_p = 4 \times 10^{18} \ atm$. Assuming $P_{X_3} \gg P_{X_6}$ and the total pressure is $10 \ atm$,the partial pressure of $X_6$ will be: