For the reaction 2 H2S(g) D 2 H2 (g) + S2 (g), Kp = 1.5 × 10−5 at 800.0°C. If the initial partial pressures of H2 and S2 in a closed container are 4.00 atm and 2.00 atm, respectively, what is the approximate equilibrium partial pressure of H2S?

The approximate equilibrium partial pressure of is 3.92  atm

Explanation:

Equilibrium constant is the ratio of the concentration of products to the concentration of reactants each term raised to its stochiometric coefficients.

The given balanced equilibrium reaction is,

On reversing the reaction:

initial pressure  4.00atm    2.00 atm       0

eqm          (4.00-2x)atm      (2.00-x) atm      2x atm

Thus approximate equilibrium partial pressure of is 3.92 atm

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