A student ran the following reaction in the laboratory at 656 K: 2NH3 (9) N₂(g) + 3H₂(g) When she introduced 0.0783 moles of NH3(g) into a 1.00 liter container, she found the equilibrium concentration of H₂(g) to be 0.108 M. Calculate the equilibrium constant, Kc, she obtained for this reaction. Kc = this question.
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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
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![**Transcription:**
A student ran the following reaction in the laboratory at 656 K:
\[ 2\text{NH}_3 (g) \rightleftharpoons \text{N}_2 (g) + 3\text{H}_2 (g) \]
When she introduced 0.0783 moles of \(\text{NH}_3 (g)\) into a 1.00 liter container, she found the equilibrium concentration of \(\text{H}_2 (g)\) to be 0.108 M.
Calculate the equilibrium constant, \( K_c \), she obtained for this reaction.
\[ K_c = \]](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2Fb8d8ce1c-d1ae-4fbf-bbe3-121c6915374e%2F3f42eaad-4ffa-460a-b626-06e2a9b8cc50%2Fh8xb07s_processed.jpeg&w=3840&q=75)
Ammonia decomposes into nitrogen and hydrogen. The equation for the balanced chemical reaction is as follows:
2NH3(g) ⇌ N2(g) + 3H2(g)
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