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
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.
Frequently Asked Questions
What scientific concept do you need to know in order to solve this problem?
Our tutors have indicated that to solve this problem you will need to apply the Hess's Law concept. You can view video lessons to learn Hess's Law. Or if you need more Hess's Law practice, you can also practice Hess's Law practice problems.
What professor is this problem relevant for?
Based on our data, we think this problem is relevant for Professor Cummings & Goldsby & McCoy's class at FSU.
What textbook is this problem found in?
Our data indicates that this problem or a close variation was asked in Chemistry - OpenStax 2015th Edition. You can also practice Chemistry - OpenStax 2015th Edition practice problems.