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Answer : The equilibrium constant for the reaction is, 0.1133
Explanation :
First we have to calculate the concentration of .
Now we have to calculate the dissociated concentration of .
The balanced equilibrium reaction is,
Initial conc. 1.731 M 0
At eqm. conc. (1.731-x) (2x) M
As we are given,
The percent of dissociation of =
= 1.2 %
So, the dissociate concentration of =
The value of x = 0.2077 M
Now we have to calculate the concentration of at equilibrium.
Concentration of = 1.731 - x = 1.731 - 0.2077 = 1.5233 M
Concentration of = 2x = 2 × 0.2077 = 0.4154 M
Now we have to calculate the equilibrium constant for the reaction.
The expression of equilibrium constant for the reaction will be :
Now put all the values in this expression, we get :
Therefore, the equilibrium constant for the reaction is, 0.1133