Question

Hydrogen and chlorine react to form hydrogen chloride, like this:

H2(g) + Cl,(g) → 2 HCl(g)
Also, a chemist finds that at a certain temperature the equilibrium mixture of hydrogen, chlorine, and hydrogen chloride has the following composition:
compound pressure at equilibrium
H2 0.78
Cl2 1.2M
HCl 1.6M
Calculate the value of the equilibrium constant for this reaction. Round your answer to significant digits.

Answer 1

Answer: The value of the equilibrium constant for this reaction is 2.7

Step-by-step explanation:

Equilibrium constant is defined as the ratio of concentration of products to the concentration of reactants each raised to the power their stoichiometric ratios. It is expressed as
`K_c`

For the given chemical reaction:

`H_2(g)+Cl_2(g)\rightarrow 2HCl(g)`

The expression for
`K_c` is written as:

`K_c=([HCl]^2)/([H_2]^1[I_2]^1)`

`K_c=((1.6)^2)/((0.78)^1* (1.2)^1)`

`K_c=2.7`

Thus the value of the equilibrium constant for this reaction is 2.7