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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.

Respuesta :

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

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 [tex]K_c[/tex]  

For the given chemical reaction:

[tex]H_2(g)+Cl_2(g)\rightarrow 2HCl(g)[/tex]

The expression for [tex]K_c[/tex] is written as:

[tex]K_c=\frac{[HCl]^2}{[H_2]^1[I_2]^1}[/tex]

[tex]K_c=\frac{(1.6)^2}{(0.78)^1\times (1.2)^1}[/tex]

[tex]K_c=2.7[/tex]

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