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 :

in scientific notation, the value of the  speed of light in a vacuum

  will be written as 2.995 * 10^8. when this value is represented in the form of

  a * 10^b, then, a = 2.995 and b = 8.

the value of the speed of light in a vacuum given above can also be rounded up to approximately 300000000. in this case, the scientific notation will be written as 3 *10^8.