Suppose 15.00 g of solid ammonium hydrogen sulfide is introduced into a 500.-mL flask at 25°C, the flask is sealed, and the system is allowed to reach equilibrium. At equilibrium, there is 0.021 mole of ammonium gas. What is the equilibrium constant, Kc, for the following reaction at 25°C? Please report 3 decimal places, without units. NH4HS(s) NH3(g) + H2S(g)
Suppose 15.00 g of solid ammonium hydrogen sulfide is introduced into a 500.-mL flask at 25°C, the flask is sealed, and the system is allowed to reach equilibrium. At equilibrium, there is 0.021 mole of ammonium gas. What is the equilibrium constant, Kc, for the following reaction at 25°C? Please report 3 decimal places, without units. NH4HS(s) NH3(g) + H2S(g)
Chapter13: Chemical Equilibrium
Section: Chapter Questions
Problem 13Q: Suppose a reaction has the equilibrium constant K = 1.3 108. What does the magnitude of this...
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Suppose 15.00 g of solid ammonium hydrogen sulfide is introduced into a 500.-mL flask at 25°C, the flask is sealed, and the system is allowed to reach equilibrium. At equilibrium, there is 0.021 mole of ammonium gas. What is the equilibrium constant, Kc, for the following reaction at 25°C? Please report 3 decimal places, without units. |
NH4HS(s) NH3(g) + H2S(g) |
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