2) Write a balanced equation for the oxidation of ammonium ion by atmospheric oxygen to nitrate ion inan acidic medium. Note that there are microorganisms (e.g., ammonia oxidizing bacteria) thatefficiently carry out this reaction in natural waters.loration oCWhat does the [F1 reveal about a drinking water source?

A Redox reaction leads to oxidation and reduction processes simultaneously. Oxidation and reduction…

Answered: 2) Write a balanced equation for the…

Chemistry: Principles and Reactions

8th Edition

ISBN:9781305079373

Author:William L. Masterton, Cecile N. Hurley

Publisher:William L. Masterton, Cecile N. Hurley

Chapter21: Chemistry Of The Nonmetals

Section: Chapter Questions

Problem 16QAP

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Calcium metal can be obtained by the direct electrolysis of molten CaCl2, at a voltage of 3.2 V. (a) How many joules of electrical energy are required to obtain 12.0 1b of calcium? (b) What is the cost of the electrical energy obtained in (a) if electrical energy is sold at the rate of nine cents per kilowatt hour?
Why is oxygen central to the existence of animal life? Use reactions to explain.
How do you write a net ionic equation for the formation of gas ex Al2(SO4)3(NH4)2SO4 •24 H2O + NaOH --> ?
(3) äg الفصل الأول 120 مقررالي الدراسية Phosphorous acid upon thermal decomposition yields phosphoric acid Phosphorus pentoxide a O Phosphine .b O Phosphorus.c Water d
What are the uses of KMnO4?
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12:07 & 3 ull 78% Possibly useful info 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 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…
(a) Write the definition of reduction and oxidation. (b) Ammonia oxidizing bacteria (AOB) play an important role in nitrogen cycle. They are also utilized in engineered systems to remove ammonia in wastewater treatment. They obtain energy by oxidizing ammonia NH3 into nitrite (NO2-) and reducing oxygen to water. Balance the reduction and oxidation reactions driven by AOB. (c) Combine the redox reactions into a single reaction. (d) Find ΔG° for the combined reaction. (e) Find ΔG for the given conditions: [NH3] = 2.7 × 10-3 M; pO2 = 0.21 atm; [NO2-] = 1.2 × 10-5 M. If necessary assumeneutral pH (i.e., pH = 7). Are the given conditions favourable for AOB growth?
Equal length of magnesium ribben are taken in two test tubes ‘A’ and ‘B\ H2SO4 is added to test tube ‘A’ and H2CO3 in the test tube ‘B’ in equal amounts:(a) Identify the test tube showing vigorous reaction.(b) Give reason to support your answer.(c) Name the gas liberated in both the tubes. How will you prove its liberation?(d) Write chemical equations for both reactions.(e) Out of the two acids taken above(i) which one will have lower pH value.(ii) lowerH+ concentration respectively.
2. An effluent waste stream contains 3300mg/L organic matter ((CH2O) suspended and dissolved) and 27mg / L ammonium ion NH4+ (as N). Write chemical equations for the complete oxidation of (CH2O) and NH4+ and calculate the total BOD of this effluent in mg/L O2
b) A solution of chlorine in water is used as a disinfectant. The equation below indicates the reaction between chlorine and water. Ch+H;O- i) > Cl+ CIO+ 2H Give a balanced equation for the reaction that occurs when a concentrated solution of NaOH is added to this medium. What name is given to this type of reaction. ii) iii) A) Write balanced equations for the preparation ofHF and HI from CaF, and Nal respectively. B) Explain any similarity or difference in the methods of preparation of HF and HI.
MASS-VOLUME 1. What is the mass of calcium carbonate must be heated to form 200 L of carbon dioxide? 2. 230 g of sodium metal was dropped in a known amount of cold water. Determine the amount of hydrogen gas in terms of volume that is produced in this reaction. 3. What volume of hydrogen at STP will be produced by the electrolysis of 180 g water? 4. Zinc sulfide reacts with oxygen to give zinc oxide and sulfur dioxide. What volume at STP of SO₂ will be given off by 435 g of zinc sulfide? 5. 2 g of sulfur is burned in oxygen. How many liters at STP of sulfur dioxide was formed?

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