N2O4(g) leftharpoons 2NO2(g); Kc=5.7 × 10-9 at 298 K At equilibrium

Question

N2O4(g) leftharpoons 2NO2(g); Kc=5.7 × 10-9 at 298 K At equilibrium (A) concentration of NO2 is higher than that of N2O4 (B) concentration of N2O4 is higher than that of NO2 (C) both N2O4 and NO2 have same concentration (D) concentration of N2O4 and NO2 keeps on changing

Tardigrade Admin · Accepted Answer

Smaller value of equilibrium constant (< 10-3) signifies the greater concentration of reactants as compared to that of products.

Q. $N_{2} O_{4 (g)} ⇌ 2 N O_{2 (g)}$ ; $K_{c} = 5.7 \times 1 0^{- 9}$ at $298 K$ At equilibrium

concentration of $N O_{2}$ is higher than that of $N_{2} O_{4}$

concentration of $N_{2} O_{4}$ is higher than that of $N O_{2}$

both $N_{2} O_{4}$ and $N O_{2}$ have same concentration

concentration of $N_{2} O_{4}$ and $N O_{2}$ keeps on changing

Smaller value of equilibrium constant $(< 1 0^{- 3})$ signifies the greater concentration of reactants as compared to that of products.

Q. N2​O4(g)​⇌2NO2(g)​; Kc​=5.7×10−9 at 298K At equilibrium

concentration of NO2​ is higher than that of N2​O4​

concentration of N2​O4​ is higher than that of NO2​

both N2​O4​ and NO2​ have same concentration

concentration of N2​O4​ and NO2​ keeps on changing