Question

The following concentrations were obtained for the formation of $NH_3(g)$ from $N_2(g)$ and $H_2(g)$ at equilibrium and at 500K: $[N_2] 1×10^{-2} M, [H_2] -2×10^{-2} M$ and $[NH_3]=2×10^{-2} M$. The equilibrium constant, K., for the reaction
$N_2(g)+3H_2(g)2NH; (g)$ at 500K is

• A. $5 x 10^3 mol^{-2}dm^6$
• B. $1 x 10^3 mol^{-2}dm^6$
• C. $5 x 10^{-3} mol^{-2}dm^6$
• D. $ 2 x 10^3 mol^{-2}dm^6$
• E. $2 x 10^{-3} mol^{-2}dm^6$

Answer 1

The Correct Option is C

The correct option is (C) : $5 x 10^{-3} mol^{-2}dm^6$