At a certain temperature, the Kp for the decomposition of H2S is 0.754. Initially, only H2S is present at a pressure of 0.139 atm in a closed container. What is the total pressure in the container at equilibrium?
The decomposition of H2S happens in the following reaction scheme.
It is given that the equilibrium constant Kp is
For a generic reaction of gases.
The expression of Kp in terms of the partial pressure of the reactant and products at equilibrium is
For us initial partial pressure of H2S = 0.139 atm. There are no H2 or S2 present initially.
We can create an ICE table to determine the equilibrium partial pressures of all species.
Initial, atm | 0.139 | 0 | 0 |
Change, atm | -2x | +2x | +x |
Equilibrium, atm | 0.139-2x | 2x | x |
Hence, the Kp expression for our equilibrium is
Hence, total pressure at equilibrium is
At a certain temperature, the Kp for the decomposition of H2S is 0.754. Initially, only H2S...
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