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Determine Equilibrium Partial Pressure

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An evacuated 4.0 L vessel containing solid sulfur is initially charged with 1.30 atm hydrogen gas at 44.9 celsius. Eventually, the following equilibrium is achieved:

H_2(gas)+ S(solid) = H_2S (gas)

Determine the equilibrium partial pressure of molecular hydrogen in the vessel given that K=0.68 for the reaction as written.

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Solution Summary

This answer is found by setting up an ICE table (initial, change, equilibrium) then solving for x. The solution includes table, calculations and answer.

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Determining Equilibrium and Partial Pressure: Example Problem

Kp = 7.69 at 830C for 2SO3 = 2SO2 + O2. If a vessel at this temperature initially contained pure sulfur dioxide and if the partial pressure of sulfur trioxide = 0.100 atm, what is the partial products in the flask at equilibrium.

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