Question

Below are the reduction half reactions for chemolithoautotrophic denitrification, where hydrogen is a source of electrons and energy and nitrate is the terminal electron acceptor.
NO3- + 10e- -> N2 (E0 = +0.74 V)
H+ + 2e- -> H2 (E0 = -0.42 V)
If you balance and combine the reactions so that 90 moles of H2 gas are oxidized to H+, how many moles of N2 gas will be produced?

Answer 1

39462 KJ of Gibbs free energy will produce. Number of moles of nitrogen = 90 moles, E0 = 0.74 + (  - 0.42) = 0.74  - 0.42 = 0.32

What is a Balanced chemical equation?

A balanced chemical equation has the same number of reactants and products. We can balance a chemical equation by adding a number to adding the same number of molecules on both sides.

In this equation,

10NO3 + 10 e - -> 5N2

4H + 2 e - -> 2H2

In this equation, 5 moles of N2 and 2 moles of Hydrogen are produced.

5 * 0.74 = 3.7 V

2 * (  -0.42) = - 0.84 V

ΔG = -nFΔE,

where F = 96.48 kJ (mol e-)

           = 90 * 96.48 * (3.7 + 0.84)

           = 90* 96.48* 4.54

            = 39462 KJ

Therefore, 39462 KJ of Gibbs free energy will produce. Number of moles of nitrogen = 90 moles, E0 = 0.74 + (  - 0.42) = 0.74  - 0.42 = 0.32.

To learn more about nitrogen, refer to the link:

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