. Calculate the equilibrium constant for the following reaction, if [NH3] = 2.78 x 10-3 M, [N₂] = 4.66 x 102 M and [H₂] = 5.18 x 10-3 a. N₂(g) + 3 H₂(g) <--> 2 NH3(8) b. Calculate K for 6 NH3(g) <--> 3 N₂(g) + 9 H₂(g)
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Chemical equilibrium and ionic equilibrium are two major concepts in chemistry. Ionic equilibrium deals with the equilibrium involved in an ionization process while chemical equilibrium deals with the equilibrium during a chemical change. Ionic equilibrium is established between the ions and unionized species in a system. Understanding the concept of ionic equilibrium is very important to answer the questions related to certain chemical reactions in chemistry.
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Bronsted-Lowry base in inorganic chemistry is any chemical substance that can accept a proton from the other chemical substance it is reacting with.
![• Calculate the equilibrium constant for the following reaction, if
[NH3] =
= 2.78 x 10-3 M, [N₂] = 4.66 x 102 M and [H₂] = 5.18 x
10-3
a. N₂(g) + 3 H₂(g) <--> 2 NH3(8)
b. Calculate K for 6 NH3(g) <--> 3 N₂(g) + 9 H₂(8)
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Calculate Kp for the problem (5-b) above at 25°](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2Fe9525ee1-97e5-4ab3-b1e5-781839ad0e63%2F527a5642-0c53-456f-9e82-8ee9bd8be5cb%2Fzoqz7tb_processed.jpeg&w=3840&q=75)
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