The equilibrium constants $(K_C)$ of two reactions $H_2 + I_2 \rightleftharpoons 2 HI$ and $N_2 + 3 H_2 \rightleftharpoons 2 NH_3$ are $50$ and $1000$,respectively. The equilibrium constant of the reaction $N_2 + 6 HI \rightleftharpoons 2 NH_3 + 3 I_2$ is closest to

$1 \ mol$ $N_2$ and $3 \ mol$ $H_2$ are taken in a $4 \ L$ closed vessel at a constant temperature. The reaction is $N_{2(g)} + 3H_{2(g)} \rightleftharpoons 2NH_{3(g)}$. If $0.25\%$ of $N_2$ is converted into ammonia,calculate $K_c$ for this reaction and the $K_c'$ for the reaction $\frac{1}{2}N_{2(g)} + \frac{3}{2}H_{2(g)} \rightleftharpoons NH_{3(g)}$.

Three moles of $PCl_{5}$,three moles of $PCl_{3}$ and two moles of $Cl_{2}$ are taken in a closed vessel. If at equilibrium the vessel has $1.5$ moles of $PCl_{5}$,the number of moles of $PCl_{3}$ present in it is

For the reaction $A_{(g)} + 3B_{(g)} \rightleftharpoons 2C_{(g)}$ at $27 \, ^oC$,$2 \, moles$ of $A$,$4 \, moles$ of $B$ and $6 \, moles$ of $C$ are present in a $2 \, litre$ vessel. If $K_C$ for the reaction is $1.2$,the reaction will proceed in

In a $10 \ L$ vessel,$1 \ mol$ each of $PCl_5$ and $PCl_3$ are present. If the vessel is heated,some $PCl_5$ dissociates. What are the concentrations of $PCl_5$,$PCl_3$,and $Cl_2$ at equilibrium,respectively?

At $T$ $(K)$,the equilibrium constant for the reaction $H_{2(g)} + Br_{2(g)} \rightleftharpoons 2 HBr_{(g)}$ is $1.6 \times 10^5$. If $10 \ bar$ of $HBr$ is introduced into a sealed vessel at $T$ $(K)$,the equilibrium pressure of $HBr$ (in $bar$) is approximately