Consider the following reaction: NH4HS(s)=NH3(g)+H2S(g)NH4HS(s)=NH3(g)+H2S(g) An equilibrium mixture of this reaction at a certain temperature was found to have [NH3]=[NH3]= 0.274 MM and [H2S]=[H2S]= 0.350 MM. What is the value of the equilibrium constant (Kc)(Kc) at this temperature?
Consider the following reaction: NH4HS(s)=NH3(g)+H2S(g)NH4HS(s)=NH3(g)+H2S(g) An equilibrium mixture of this reaction at a certain temperature was found to have [NH3]=[NH3]= 0.274 MM and [H2S]=[H2S]= 0.350 MM. What is the value of the equilibrium constant (Kc)(Kc) at this temperature?
Chemistry: Matter and Change
1st Edition
ISBN:9780078746376
Author:Dinah Zike, Laurel Dingrando, Nicholas Hainen, Cheryl Wistrom
Publisher:Dinah Zike, Laurel Dingrando, Nicholas Hainen, Cheryl Wistrom
Chapter17: Chemical Equilibrium
Section: Chapter Questions
Problem 39A
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![Consider the following reaction:
NH4HS(s)=NH3(g)+H2S(g)NH4HS(s)=NH3(g)+H2S(g)
An equilibrium mixture of this reaction at a certain temperature was found to have [NH3]=[NH3]=
0.274 MM and [H2S]=[H2S]= 0.350 MM.
What is the value of the equilibrium constant (Kc)(Kc) at this temperature?](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2F16bcf46e-2bc9-4589-8427-017f68b5680b%2F40874660-bb9a-4bb5-ab3c-1c431f102413%2F4xhpkpb_processed.jpeg&w=3840&q=75)
Transcribed Image Text:Consider the following reaction:
NH4HS(s)=NH3(g)+H2S(g)NH4HS(s)=NH3(g)+H2S(g)
An equilibrium mixture of this reaction at a certain temperature was found to have [NH3]=[NH3]=
0.274 MM and [H2S]=[H2S]= 0.350 MM.
What is the value of the equilibrium constant (Kc)(Kc) at this temperature?
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