Assume that the reaction for the formation of gaseous hydrogen fluoride from hydrogen and fluorine has an equilibrium constant of 1.15 X 102 at a certain temperature. In a particular experiment, 3.00 mole of each component was added to a 1.50 L flask. Calculate the equilibrium concentrations of all species.

The equilibrium concentrations of all species :

Explanation:

Moles of hydrogen gas = 3.00 mole

Concentration of hydrogen gas =

Moles of fluorine gas = 3.00 mole

Concentration of fluorine gas =

Given the equilibrium constant of the reaction =

Initial

2.0 M  2.0 M     0

At equilibrium

(2.0-x)M  (2.0 -x)M         2x

An expression of is given by :

On solving for x , we get :

x = 1.686 M

The equilibrium concentrations of all species :

може ли да зареждате повече информация, моля

a. energy is absorbed in the reaction.

if in a given reaction the energy of products is greater than the energy of reactants it means that reaction is endothermic and during the reaction, the energy is absorbed by reactants. in an endothermic reaction, the products have more stored chemical energy than the reactants. and in this reaction the reactants are more stable than products before the compounds with less energy are always more stable.