Ammonia (NH3) is naturally produced through the decomposition of organic material as well as being high in wastewater discharged to natural waters. In the environment it is oxidized to form nitrite (NO2-), and nitrite is then oxidized to form nitrate (NO3-) in a process called nitrification. The balanced equations are given below: 2NH3 + 3O2 → 2NO2- + 2H+ + 2H20 2NO2- + O2 → 2NO3- a) Assuming complete oxidation, what is the theoretical oxygen demand to convert 100mg/L of ammonia to nitrate (i.e., how much oxygen is necessary)? Report your answer as mg/L of O2. Answer: 376 mg/L O2 b) This conversion process makes water more acidic. With reference to the equations for pH, explain why this occurs
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.
Ammonia (NH3) is naturally produced through the decomposition of organic material as well
as being high in wastewater discharged to natural waters. In the environment it is oxidized
to form nitrite (NO2-), and nitrite is then oxidized to form nitrate (NO3-) in a process called
nitrification. The balanced equations are given below:
2NH3 + 3O2 → 2NO2- + 2H+ + 2H20
2NO2- + O2 → 2NO3-
a) Assuming complete oxidation, what is the theoretical oxygen demand to convert
100mg/L of ammonia to nitrate (i.e., how much oxygen is necessary)? Report your
answer as mg/L of O2.
Answer: 376 mg/L O2
b) This conversion process makes water more acidic. With reference to the equations for
pH, explain why this occurs
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