The equilibrium constants of the following are:

$\begin{cases}{N}_{2} + 3{H}_{2} ⇌ 2{NH}_{3} & {K}_{1} \\ {N}_{2} + {O}_{2} ⇌ 2NO & {K}_{2} \\ {H}_{2} + \dfrac{1}{2}{O}_{2} \to {H}_{2}O & {K}_{3}\end{cases}$

The equilibrium constant ( $K$ ) of the reaction:

$2N H{}_{3} + \dfrac{5}{2}O{}_{2}\overset{K }{⇌}2N O + 3H{}_{2}O$ , will be:

Question

The equilibrium constants of the following are:

\begin{cases}{N}_{2} + 3{H}_{2} ⇌ 2{NH}_{3} & {K}_{1} \\ {N}_{2} + {O}_{2} ⇌ 2NO & {K}_{2} \\ {H}_{2} + \dfrac{1}{2}{O}_{2} \to {H}_{2}O & {K}_{3}\end{cases}

The equilibrium constant (

K

) of the reaction:

2N H{}_{3} + \dfrac{5}{2}O{}_{2}\overset{K }{⇌}2N O + 3H{}_{2}O

, will be:

Quantrex Academy · Accepted Answer

Correct answer: B. K _ 2 K _ 3 ^ 3 K _ 1

(I) N _ 2 + 3 H _ 2 ⇌ 2 NH _ 3 ; K _ 1 = [ NH _ 3 ] ^ 2 [ N _ 2 ] [ H _ 2 ] ^ 3 (II) N _ 2 + O _ 2 ⇌ 2NO; K _ 2 = [NO] ^ 2 [ N _ 2 ][ O _ 2 ] (III) H _ 2 + (1)/(2) O _ 2 → H _ 2 O; K _ 3 = [ H _ 2 O] [ H _ 2 ][ O _ 2 ](1)/(2) (II + 3 × III - I) will give 2N H _ 3 + (5)/(2)O _ 2 K ⇌ 2N O + 3H _ 2 O ; ∴ K = K _ 2 × K _ 3 ^ 3 K _ 1

The equilibrium constants of the following are: cases N _ 2 + 3 H _...

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