What is the relationship between the equilibrium constants for reactions 1, 2, and 3? K₁ Reaction 1: H₂CO3(aq) + H₂O(1) ⇒ HCO3¯(aq) + H3O+ (aq) K₂ Reaction 2: HCO3(aq) + H₂O(1) ⇒ CO3²−(aq) + H3O+(1) K3 Reaction 3: CO3²-(aq) + H₂CO3(aq) = 2HCO3(aq) K3 = K₁ + K₂ O K3 = K2/K₁ K3 = K₁/K₂ O K3 = KiK2
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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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HELP
![What is the relationship between the equilibrium constants for reactions 1,
2, and 3?
Reaction 1: H₂CO3(aq) + H₂O(1) ⇒ HCO3¯(aq) + H3O+(aq)
K₁
K₂
Reaction 2: HCO3¯(aq) + H₂O(1) ⇒ CO3²−(aq) + H3O+(1)
Reaction 3: CO32-(aq) + H₂CO3(aq) → 2HCO3(aq)
K3
K3 = K₁ + K₂
O K3 = K2/K1
OK₁=K₁/K₂
O K3 = K₁K₂
Here are the equilibrium constants for two reactions of nitrogen with
oxygen. What is the equilibrium constant for N₂O (g) + 1/2O₂(g) → 2NO
(g)? Express your answer completely. Do not use scientific notation in
writing your answer. For example, write 1000 instead of 1 x 10³. Express
your answer in two significant figures.
N₂(g) + O₂(g) = 2NO(g)
N₂(g) + 1/2O₂(g) = N₂O(g)
K= 4.1 × 10-31
K=2.4 × 10-18](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2F051200d1-e1bb-4e0b-81dd-1dbfe17d71aa%2Fe6d2dbac-0080-451a-abe2-1df1b866e0d3%2F8cfadml_processed.png&w=3840&q=75)
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Here are the equilibrium constants for two reactions of nitrogen with oxygen. What is the equilibrium constant for N₂O (g) + 1/2O₂(g) → 2NO (g)?
N₂(g) + O₂(g) = 2NO(g) K= 4.1 × 10^-31
N₂(g) + 1/2O₂(g) = N₂O(g) K=2.4 × 10^-18
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