For the reaction $CO_{(g)} + Cl_{2(g)} \rightleftharpoons COCl_{2(g)}$,$\frac{K_p}{K_c}$ is equal to

The equilibrium constant at $850 \ K$ for the reaction $N_{2(g)} + O_{2(g)} \rightleftharpoons 2 NO_{(g)}$ is $0.5625$. The equilibrium concentration of $NO_{(g)}$ is $3.0 \times 10^{-3} \ M$. If the equilibrium concentrations of $N_{2(g)}$ and $O_{2(g)}$ are equal,the concentration of $N_{2(g)}$ in $M$ is

For the reaction $2NOBr_{(g)} \rightleftharpoons 2NO_{(g)} + Br_{2(g)}$,if $P_{Br_2} = \frac{P}{9}$ at equilibrium and $P$ is the total pressure,find the value of $\frac{K_P}{P}$.

For the reaction $A_{(g)} + 2B_{(g)} \rightleftharpoons 2C_{(g)}$,$1 \ mol$ of $A$ and $1.5 \ mol$ of $B$ are taken in a $2 \ L$ vessel. If the concentration of $C$ at equilibrium is $0.35 \ M$,then the equilibrium constant $K_c$ of the reaction will be ....... $M^{-1}$.

For which of the following reactions is $K_c \leq K_p$ at $298 \ K$?

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?