For the reaction $3A_{(g)} + B_{(g)} \rightleftharpoons 2C_{(g)}$ at a given temperature,$K_c$ is $9.0$. What must be the volume of the flask if a mixture of $2.0 \ mol$ each of $A, B$ and $C$ is obtained at equilibrium? .....$L$

$1.1 \ mol$ of $A$ and $2.2 \ mol$ of $B$ are mixed in a $1 \ L$ flask until equilibrium is reached. At equilibrium,$0.2 \ mol$ of $C$ is formed. If the equilibrium reaction is $A + 2B \rightleftharpoons 2C + D$,the value of the equilibrium constant $K_C$ is:

Given the equilibria:
$I: A + 2B \rightleftharpoons C ; K_{eq} = K_1$
$II: C + D \rightleftharpoons 3A ; K_{eq} = K_2$
$III: 6B + D \rightleftharpoons 2C ; K_{eq} = K_3$
Which of the following relations is correct?

For the reaction $C_{(s)} + CO_{2(g)} \rightleftharpoons 2CO_{(g)}$,the partial pressures of $CO_2$ and $CO$ are $2.0 \ atm$ and $4.0 \ atm$ respectively. The value of $K_p$ for the reaction is ............ .

For the reaction $SO_{3(g)} \rightleftharpoons SO_{2(g)} + \frac{1}{2}O_{2(g)}$,the equilibrium constant $K_C = 4.9 \times 10^{-2}$. Calculate the $K_C$ for the reaction $2SO_{2(g)} + O_{2(g)} \rightleftharpoons 2SO_{3(g)}$.

For the reactions $(i) \ N_{2(g)} + 3H_{2(g)} \rightleftharpoons 2NH_{3(g)}$ and $(ii) \ \frac{1}{2}N_{2(g)} + \frac{3}{2}H_{2(g)} \rightleftharpoons NH_{3(g)}$,if their equilibrium constants are $K_c(1)$ and $K_c(2)$ respectively,what is the relation between them?