4NH3(g) +50₂(g) = 4NO(g) + 6H₂O(g) ΔΗ° = -1000. kJ K = 1.35 When the reaction is altered as below, what is the value of the enthalpy, AH°? 2NO(g) + 3H₂O(g) = 2NH3(g) + O₂(g) ΔΗ° = [ ? ] kJ Include either a + or - sign AND the magnitude in your answer. Enthalpy (kJ) Enter
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.
![**Chemical Reaction Enthalpy Calculation**
For the following chemical reaction:
\[ 4\text{NH}_3(g) + 5\text{O}_2(g) \rightleftharpoons 4\text{NO}(g) + 6\text{H}_2\text{O}(g) \]
\[ \Delta H^\circ = -1000. \text{kJ} \quad K = 1.35 \]
When the reaction is modified as shown below, what is the value of the standard enthalpy change, \(\Delta H^\circ\)?
\[ 2\text{NO}(g) + 3\text{H}_2\text{O}(g) \rightleftharpoons 2\text{NH}_3(g) + \frac{5}{2}\text{O}_2(g) \]
\[ \Delta H^\circ = \boxed{?} \text{kJ} \]
**Note:** Include either a \( + \) or \( - \) sign AND the magnitude in your answer.
[Input Field for Enthalpy (kJ)]
[Enter Button]
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**Explanation:**
- The initial reaction equation and its associated enthalpy change and equilibrium constant are provided.
- You are asked to determine the enthalpy change for a modified version of this reaction.
- You need to calculate the new value for \(\Delta H^\circ\) based on the given information.
- Ensure to indicate whether the enthalpy change is positive or negative, and specify the magnitude accurately.](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2F491b4bae-792a-4f14-88e8-39a4bfb5b6ad%2F0c1fc7f3-f3b0-40fa-bade-61099c18604e%2Fy44v6e_processed.jpeg&w=3840&q=75)
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