Hydrogen chloride decomposes to form hydrogen and chlorine, like this: 2HCl(g) + H2(g) â Cl2(g)

Also, a chemist finds that at a certain temperature the equilibrium mixture of hydrogen chloride, hydrogen, and chlorine has the following composition:

compound pressure at equilibrium
HCl 84.4 atm
H2 77.9 atm
Cl2 54.4

Required:
Calculate the value of the equilibrium constant for this reaction. Round your answer to significant digits.

Solution :

Given :

Partial pressure of HCl, = 84.4 atm

Partial pressure of , = 77.9 atm

Partial pressure of , = 54.4 atm

Reaction :

Using equilibrium concept,

 (in 2 significant figures)

or

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your answer is a. the enthalpy of formation for a pure element in its standard state is always positive.