The first two steps in the industrial synthesis of nitric acid produce nitrogen dioxide from ammonia: 4 NH3(g) +50₂ (g) 4 NO(g) + 6H₂O(g) = K₁ K₂ 2 NO(g) + O₂(g) 2 NO₂ (g). The net reaction is: K 4 NH3(g) +70₂ (g) 4NO₂(g) + 6H₂O(g) Write an equation that gives the overall equilibrium constant K in terms of the equilibrium constants K, and K₂. If you need to include any physical constants, be sure you use their standard symbols, which you'll find in the ALEKS Calculator. K = ロ・ロ 00 010 X 09 S ?
Thermochemistry
Thermochemistry can be considered as a branch of thermodynamics that deals with the connections between warmth, work, and various types of energy, formed because of different synthetic and actual cycles. Thermochemistry describes the energy changes that occur as a result of reactions or chemical changes in a substance.
Exergonic Reaction
The term exergonic is derived from the Greek word in which ‘ergon’ means work and exergonic means ‘work outside’. Exergonic reactions releases work energy. Exergonic reactions are different from exothermic reactions, the one that releases only heat energy during the course of the reaction. So, exothermic reaction is one type of exergonic reaction. Exergonic reaction releases work energy in different forms like heat, light or sound. For example, a glow stick releases light making that an exergonic reaction and not an exothermic reaction since no heat is released. Even endothermic reactions at very high temperature are exergonic.
![**Title: Industrial Synthesis of Nitric Acid: Nitrogen Dioxide Production**
The first two steps in the industrial synthesis of nitric acid produce nitrogen dioxide from ammonia:
1. \( 4 \text{NH}_3 (g) + 5 \text{O}_2 (g) \rightleftharpoons 4 \text{NO} (g) + 6 \text{H}_2\text{O} (g) \)
Equilibrium constant: \( K_1 \)
2. \( 2 \text{NO} (g) + \text{O}_2 (g) \rightleftharpoons 2 \text{NO}_2 (g) \)
Equilibrium constant: \( K_2 \)
The net reaction is:
\[ 4 \text{NH}_3 (g) + 7 \text{O}_2 (g) \rightleftharpoons 4 \text{NO}_2 (g) + 6 \text{H}_2\text{O} (g) \]
Equilibrium constant: \( K \)
**Objective:**
Write an equation that gives the overall equilibrium constant \( K \) in terms of the equilibrium constants \( K_1 \) and \( K_2 \). Ensure to use their standard symbols, which you'll find in the ALEKS Calculator.
**Box for Answer:**
\[ K = \]
**Explanation:**
To find the overall equilibrium constant \( K \) for the net reaction, you need to combine the equilibrium constants of the individual steps, \( K_1 \) and \( K_2 \). In this case, the overall equilibrium constant \( K \) can be expressed as the product of \( K_1 \) and \( K_2 \).
Thus:
\[ K = K_1 \times K_2 \]
Given this understanding, please enter the correct expression for \( K \) using the ALEKS Calculator symbols.](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2Fe361a5c2-e3a6-4cd8-bee8-5dcb720cb10b%2F8bf97f6d-f0bb-4c2e-9af1-109b8d14fb09%2F1wcqmin_processed.jpeg&w=3840&q=75)
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