In the reaction $A + 2B \rightleftharpoons 2C$,if $2$ moles of $A$,$3.0$ moles of $B$ and $2.0$ moles of $C$ are placed in a $2.0 \ L$ flask and the equilibrium concentration of $C$ is $0.5 \ mol/L$. The equilibrium constant $K_c$ for the reaction is:

Consider the following liquid-vapour equilibrium.
$Liquid \rightleftharpoons Vapour$
Which of the following relations is correct?

At a certain temperature,the equilibrium constant $(K_C)$ is $16$ for the reaction:
$SO_2(g) + NO_2(g) \rightleftharpoons SO_3(g) + NO(g)$
If we take one mole of each of the four gases in a $1 \ L$ container,what would be the equilibrium concentration of $NO$ and $NO_2$ respectively?

Which of the following statements regarding a chemical equilibrium is wrong?

At $T(K)$,the $K_p$ for the reaction $A_2B_{6(g)} \rightleftharpoons A_2B_{4(g)} + B_{2(g)}$ is $0.04 \text{ atm}$. The equilibrium pressure (in $\text{atm}$) of $A_2B_{6(g)}$ when it is placed in a flask at $4 \text{ atm}$ pressure and allowed to come to equilibrium is:

Given the equilibrium constants for the following three reactions:
$(1) N_2 + 3H_2 \rightleftharpoons 2NH_3; K_1$
$(2) N_2 + O_2 \rightleftharpoons 2NO; K_2$
$(3) H_2 + \frac{1}{2}O_2 \rightleftharpoons H_2O; K_3$
The equilibrium constant for the reaction of $NH_3$ with oxygen to form $NO$ and $H_2O$ is: