At $3000 \ K$ the equilibrium pressures of $CO_2$,$CO$ and $O_2$ are $0.6 \ atm$,$0.4 \ atm$ and $0.2 \ atm$ respectively. $K_p$ for the reaction,$2CO_2 \rightleftharpoons 2CO + O_2$ is

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

Equilibrium constant for the reaction $H_2O_{(g)} + CO_{(g)} \rightleftharpoons H_{2(g)} + CO_{2(g)}$ is $81$. If the velocity constant of the forward reaction is $162 \ L \ mol^{-1} \ s^{-1}$,what is the velocity constant (in $L \ mol^{-1} \ s^{-1}$) for the backward reaction?

Dihydrogen gas used in Haber's process is produced by reacting methane from natural gas with high temperature steam. The first stage of two stage reaction involves the formation of $CO$ and $H_2$. In second stage,$CO$ formed in first stage is reacted with more steam in water gas shift reaction,
$CO_{(g)} + H_2O_{(g)} \longleftrightarrow CO_{2(g)} + H_{2(g)}$
If a reaction vessel at $400^{\circ}C$ is charged with an equimolar mixture of $CO$ and steam such that $P_{CO} = P_{H_2O} = 4.0 \ bar,$ what will be the partial pressure of $H_2$ at equilibrium? $K_p = 10.1$ at $400^{\circ}C$

At $527 \ ^oC$,the reaction given below has $K_c = 4$.
$NH_{3(g)} \rightleftharpoons \frac{1}{2} N_{2(g)} + \frac{3}{2} H_{2(g)}$
What is the $K_P$ for the following reaction?
$N_{2(g)} + 3H_{2(g)} \rightleftharpoons 2NH_{3(g)}$

For a reversible reaction $A \rightleftharpoons B$,the equilibrium concentration of $B$,denoted as $[B]_e$,is given by which expression?