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equilibrium consant Kp and change of chemical equilibrium

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A 6.1589 gm sample of ammonium hydrogen sulfide is placed in a 4.00L vessel at 24 degrees Celsius. After equilibrium the total pressure inside is 0.709 atm. Some solid ammonium hydrogen sulfide remains.

What is the Kp for the reaction?

What percentage of the solid has decomposed?

If the volume of the vessel were doubled at constant temperature, what would happen to the solid in the vessel?

We just started kinetics in my class and I am confused.

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Solution Summary

The solution shows how to calculate the equilibrium constant Kp of the decomposition of NH4HS. It then explains the effect of increasing the volume of the container on the chemical equilibrium.

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If the volume of the vessel were doubled at constant temperature, what would happen to ...

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