🤓 Based on our data, we think this question is relevant for Professor Cummings & Goldsby & McCoy's class at FSU.

Solution: The following sequence of reactions occurs in the commercial production of aqueous nitric acid:4NH3(g) + 5O2(g) ⟶ 4NO(g) + 6H2O(l)           ΔH = −907 kJ2NO(g) + O2(g) ⟶ 2NO2(g)                             ΔH = −113 kJ3NO2 + H2O(l) ⟶ 2HNO3(aq) + NO(g)            ΔH = −139 kJDetermine the total energy change for the production of one mole of aqueous nitric acid by this process.

Problem

The following sequence of reactions occurs in the commercial production of aqueous nitric acid:

4NH3(g) + 5O2(g) ⟶ 4NO(g) + 6H2O(l)           ΔH = −907 kJ
2NO(g) + O2(g) ⟶ 2NO2(g)                             ΔH = −113 kJ
3NO2 + H2O(l) ⟶ 2HNO3(aq) + NO(g)            ΔH = −139 kJ

Determine the total energy change for the production of one mole of aqueous nitric acid by this process.

Solution

To find the ΔHrxn, we need to combine the three reactions where we should be getting HNO3 as product

However, the problem is asking for the energy needed to produce 1 mole of HNO3, and in the given 3rd reaction, we have 2 moles of HNO3

We will be dividing the final ΔH calculated by 2 to get the energy needed for every 1 mol HNO3 produced

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