eeq/mole cells Nitrogen Source AGpe (kJ/g cells) AGpe (kJ/eeq cells) Ammonium (NH,") Nitrate (NO3) 20 3.33 18.8 28 3.33 13.5 Nitrite (NO2) 26 3.33 14.5 Dinitrogen (N2) 23 3.33 16.4 R = fe Re + f, Rs R= fe (Ra - Ra) + fs (Rc- Ra) So R = fe Ra + fs Rc - Rd (Note that -Rd denotes that the direction of the reaction is the opposite of that reported in the Rittmann/McCarty tables) Also note
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.
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eeq/mole
cells
Nitrogen Source
AGpe (kJ/g
cells)
3.33
AGpe (kJ/eeq
cells)
Ammonium (NH,")
Nitrate (NO;)
Nitrite (NO2")
Dinitrogen (N2)
20
18.8
28
3.33
13.5
26
3.33
14.5
23
3.33
16.4
R = fe Re + f, Rs
R = fe (Ra – Rd) + fs (Rc – Rd)
So
R = fe Ra + fs Rc – Rd
(Note that -Rd denotes that the direction of the reaction is the
opposite of that reported in the Rittmann/McCarty tables) Also note
that if the direction of a reaction is reversed, the sign on the free
energy value also changes).
Chemical
AGf
(kJ/mol)
species
AG, AG,
A =-
OH-
-198.76
ɛAG,
Toluene
n=-1if AG, <0
+114.22
(C,H3)
n=1if AG, >0
Water
-237
1
H+
-39.9
1+ A
N2
f +f° =1
Carbon
AG, = 35.09 – AG.°
Dioxide
-394
(CO2)
ɛ = 0.6
Nitrate
-111.34
(NO3)
Molecular Weights
Oxygen 16
Hydrogen 1
Nitrogen 14
Carbon 12
ΔG"ΣΔG, Products-ΣΔG, Reactants
= [(c) (AG; of C) + (d) (AG; of D)] – [(a) (AG; of A) + (b) (AG¡ of B)]
Sulfur 32
AG' = AG" + RT In [C][D]d
where: Ris the ideal gas constant 0.00829 kJ/mol-ºK
[A]°[B]»
Tis the absolute temperature (°K) and °K = °C + 273.15
[In this equation, [] represents the activity of the constituent. The activity of the solutes (aqueous
species) is close enough for our purposes to molar (M) concentration. The activity of gaseous
species (e.g. H2, O2, CO2), are entered as partial pressures in atmospheres (atm). The solvent
(typically water in our applications) is considered to have an activity of 1.]
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Here we have to write the balanced redox chemical reaction of toluene and Nitrate ion to produce CO2 ,N2 and H2O.
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