Question

Consider the reaction.

Upper H subscript 2 upper o (g) plus upper C l subscript 2 upper O (g) double-headed arrow 2 upper H upper C l upper O (g).

At equilibrium, the concentrations of the different species are as follows.

[H2O] = 0.077 M
[Cl2O] = 0.077 M
[HClO] = 0.023 M

What is the equilibrium constant for the reaction at this temperature?
0.089
0.26
3.9
11

Answer 1

Answer:

The value of Equilibrium constant for the given reaction is 0.089

Explanation:

The given data shows the following reaction

    H2O (g)  + Cl2O (g) ⇄ 2 HClO (g)

The above reaction is in equilibrium.

Equilibrium constant K  = $\frac{[C]^c*[D]^d}{[A]^a*[B]^b}$

for the reaction

aA+bB ⇆ cC +dD

so

K  = $\frac{[HClO]^2}{[H2O][Cl2O]}$

    = $\frac{[0.023]^2}{[0.077][0.077]}$ = 23*23/77*77 = 0.089

Therefore the value of Equilibrium constant for the given reaction is 0.089

Answer 2

Answer:

The value of Equilibrium constant for the given reaction is 0.089