2H 2 S (g) = 2H 2 (g) + S 2 (g) When heated hydrogen sulfide gas decomposes acco

Question

2H2S (g) = 2H2 (g) + S2 (g)

When heated hydrogen sulfide gas decomposes according to the equation above. A 3.40g smple of H2S(g) is introduced into an evacuated rigid 1.25 L container. The sealed container is heated to 483 K, and 3.72 x10-2 mol of S2 (g) is present at equilibrium.

a) Write the expression for the equilibrium constant, Kc for the decomposition reaction represented above.

b) Calculate the equilibrium concentration in M of H2 (g) and H2S (g) in the container 483 K

c) Calculate the value of the equilibrium constant Kc for the decomposition reaction of 483K

Explanation / Answer

The reaction is

                2H2S                       ----2H2                  +S2

Initial moles

                0.1                               0                         0

At equilibrium moles

                0.1-2x                       2x                        x

Given x= 3.72 x10-2 by substituting this

                0.0256                   0.0744                  0.0372

Equilibrium concentrations(moles/Volume)

                0.0256/1.25         0.0744/1.25        0.0372/1.25

                =0.02048M          0.0595M               0.02976M

Answers

A) expression for Kc = [H2]2[S2]/[H2S]2

B) equilibrium concentration of H2 = 0.0595M

    Equilibrium concentration of H2s = 0.02048M

C) Kc = (0.0595)2 (0.02976)/(0.02048)2 = 0.2513

Related Questions

Navigate

• Browse (All)
• Browse 2
• Subjects

Integrity-first tutoring: explanations and feedback only — we do not complete graded work. Learn more.