Answer:
The total energy change for the production of one mole of aqueous nitric acid is 709,8kJ
Explanation:
The three steps in the industrial production of nitric acid are:
4NH₃(g) + 5O₂(g) → 4NO(g) + 6H₂O(l) ΔH = −1166.0 kJ/mol <em>(1) </em>
2NO(g) + O₂(g) → 2NO₂(g) ΔH = −116.2 kJ/mol <em>(2) </em>
3NO₂(g) + H₂O(l) → 2HNO₃(aq) + NO(g) ΔH = −137.3 kJ/mol <em>(3)</em>
For the total process:
4NH₃(g) + 6O₂(g) + NO₂ → 3NO(g) + 2HNO₃(aq) + 5H₂O(l)
The ΔH is <em>(Hess's law) </em>: -1166,0kJ/mol - 116,2kJ/mol - 137,7kJ/mol = <em>-1419,5 kJ/mol</em>
As the total process produce two moles of nitric acid, the total energy change for the production of one mole of aqueous nitric acid is:
-1419,5 kJ/mol× = <em>709,8 kJ</em>
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I hope it helps!