Question

Match the column

The decomposition of ammonia on platinum surface follow the change,
${2NH}_3$ $⟶$ $N_2$ + ${3H}_2$ ; K = 2.5 ${10}^{-4}$ ${MS}^{-1}$ & $-\frac{d{[NH}_3]}{dt}=\frac{K_1{[NH}_3]}{1+K_2{[NH}_3]}$,
where $K_1$ and $k_2$ are constant.

Answer 1

(A) $\frac{-d{[NH}_3]}{dt}$ represents the rate of decomposition of ${NH}_3$
(B) $\frac{d{[N}_2]}{dt}$ represents the rate of formation of $N_2$
(C) $\frac{d{[H}_2]}{dt}$ represents the rate of formation of $H_2$
(D) If the decomposition is zero order, the rate of production of $N_2$ is 2.5 ${10}^{-4}$ M ${Sec}^{-1}$
(E) If the decomposition is zero order, the rate of production of $H_2$ is 7.5 ${10}^{-4}$ M ${Sec}^{-1}$
(F) the order for decomposition of ${NH}_3$ if ${[NH}_3]$ very very less is first.
(G) the order for decomposition of ${NH}_3$ if ${[NH}_3]$ very very high is zero.