posted by Anonymous on .
The decomposition of ammonium hydrogen sulfide that is shown below is an endothermic process.
NH4HS(s) reverse reaction arrow NH3(g) + H2S(g)
A 6.1589 g sample of the solid is placed in an evacuated 4.000 L vessel at exactly 24°C. After equilibrium has been established, the total pressure inside is 0.709 atm. Some solid NH4HS remains in the vessel.
a.)If the volume of the vessel were doubled at constant temperature, what would happen to the amount of solid in the vessel?
So K = p(NH3)*p(H2S)
If the volume is doubled, the pressure is halved; therefore, the reaction will shift to the right and more of the NH4HS will decompose. Thus, the solid will be decreased.