MCQ
$2$ $mol$ of ${N_2}$ is mixed with $6$ $mol$ of ${H_2}$ in a closed vessel of one litre capacity. If $50\%$ of ${N_2}$ is converted into $N{H_3}$ at equilibrium, the value of ${K_c}$ for the reaction ${N_{2(g)}} + 3{H_{2(g)}}$ $\rightleftharpoons$ $2N{H_{3(g)}}$ is
- ✓$4/27$
- B$27/4$
- C$1/27$
- D$24$
