How much heat will be released (AH) if 0.4391 mol of NHs are mixed with 0.20 mol of O2 in the following chemical reaction? 4 NHs (g) + O2 (g) 2 NaH. (g) + 2 H2O (g) AH° = -286 kJ/mol
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.
![**Transcription for Educational Website:**
**Title: Calculating Heat Release in a Chemical Reaction**
**Problem Statement:**
How much heat will be released (ΔH) if 0.4391 mol of NH₃ are mixed with 0.20 mol of O₂ in the following chemical reaction?
\[ 4 \text{NH}_3 (g) + O_2 (g) \rightarrow 2 \text{N}_2\text{H}_4 (g) + 2 \text{H}_2\text{O} (g) \]
\[ \Delta H^\circ = -286 \, \text{kJ/mol} \]
**Explanation:**
This problem involves calculating the heat release during a chemical reaction using stoichiometry and the given enthalpy change (ΔH°) per mole of reaction. Here, the enthalpy change (ΔH°) is given as -286 kJ/mol, indicating that the reaction is exothermic and releases heat.
To find out how much heat will be released specifically for the given amounts of NH₃ and O₂, we will:
1. Identify the limiting reactant from the given moles of NH₃ and O₂.
2. Use stoichiometry to determine the amount of heat released based on the moles of the limiting reactant.
This exercise helps in understanding energy changes in chemical reactions and how stoichiometry is used to calculate these changes precisely.](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2Fd862c25f-a636-4347-831e-84b629db5903%2F23d2ec6f-c42c-49cb-870f-f13318b485b9%2Fcqo4u95_processed.jpeg&w=3840&q=75)
Change in enthalpy is proportional to the number of moles of reactants and products associated with a reaction.
specifically depends on the number of moles of the reactant that gets completely consumed (limiting reactant).
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