Nitric acid can be formed in two steps from the atmospheric gases nitrogen and oxygen, plus hydrogen prepared by reforming natural gas. In the first step, nitrogen and hydrogen react to form ammonia: N₂(g) + 3H₂(g) → 2 NH3(g) AH=-92. kJ In the second step, ammonia and oxygen react to form nitric acid and water: NH3(g) + 2O₂(g) → HNO₂(g) + H₂O(g) ΔΗ= -330. kJ Calculate the net change in enthalpy for the formation of one mole of nitric acid from nitrogen, hydrogen and oxygen from these reactions. Round your answer to the nearest kJ.
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.
![### Formation of Nitric Acid
Nitric acid can be synthesized in two steps using atmospheric nitrogen and oxygen, with hydrogen derived from reformed natural gas.
**Step 1: Formation of Ammonia**
\[ \text{N}_2(g) + 3\text{H}_2(g) \rightarrow 2\text{NH}_3(g) \quad \Delta H = -92 \text{ kJ} \]
In this exothermic reaction, nitrogen gas reacts with hydrogen gas to form ammonia, releasing 92 kJ of energy.
**Step 2: Formation of Nitric Acid and Water**
\[ \text{NH}_3(g) + 2\text{O}_2(g) \rightarrow \text{HNO}_3(g) + \text{H}_2\text{O}(g) \quad \Delta H = -330 \text{ kJ} \]
Here, ammonia reacts with oxygen gas to produce nitric acid and water, with an energy release of 330 kJ.
**Objective:**
Calculate the net change in enthalpy for the formation of *one mole* of nitric acid from nitrogen, hydrogen, and oxygen. Round your answer to the nearest kJ.
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