Ch 8 Discussion Qs

Ammonia (NH3) is naturally produced through the decomposition of organic material as wellas being high in wastewater discharged to natural waters. In the environment it is oxidizedto form nitrite (NO2-), and nitrite is then oxidized to form nitrate (NO3-) in a process callednitrification. The balanced equations are given below:2NH3 + 3O2 → 2NO2- + 2H+ + 2H202NO2- + O2 → 2NO3-a) Assuming complete oxidation, what is the theoretical oxygen demand to convert100mg/L of ammonia to nitrate (i.e., how much oxygen is necessary)? Report youranswer as mg/L of O2.Answer: 376 mg/L O2b) This conversion process makes water more acidic. With reference to the equations forpH, explain why this occurs

balance the following chemical equation (if necessary):

19. The chemical equation for photosynthesis is _CO2 (g) + _H₂O (1)→ __C6H1206 (s) + (C6H12O6 is glucose, the simplest sugar) a. Balance the chemical equation above by filling in the blanks. b. According to onetreeplanted.org, the average tree (across all climates and sizes) removes 10 kg of carbon dioxide from the atmosphere every year. Based on this, what mass of glucose is produced annually by the average tree? O2 (g) c. Teak is a common species of tropical tree. The graph below shows the amount of CO₂ absorbed by teak forests in tons of CO₂ per hectare of forest per year, according to the climate region where the forests are found (dry = low rainfall, humid=high rainfall). Looking at your photosynthesis equation again, what does this data suggest about which reactant is the limiting reactant for teak trees? Explain. C Teak Carbon sequestration rate (tons CO₂ ha -1yr -1) 10 10 20 Tropical humid Tropical dry Aboveground biomass, 0-20 years Belowground biomass, 0 -20 years

7. Applying the principles of green chemistry requires some consideration of the way in which they can be applied. Figure 1 represents a generic industrial process. Using the principles of green chemistry and circled letters, describę how four of the principles could be applied to this process to make it a green operation. E kaEA product raw materials energy Source waste гeactor Figure 1 st

When potassium metal is placed in water, a large amount of energy is released as potassium hydroxide and hydrogen gas are produced in the reaction 2K(s) + 2H2O(l) → 2KOH(aq) + H2(g). Your lab partner says this is a redox reaction and a combustion reaction. Do you agree? Defend your answer by explaining whether or not it meets the requirements of each type of reaction.                   Source                  StylesFormat

Include a CLAIM: answer the question. Is this correct or not? Include EVIDENCE: Describe what you see in the calculation work that supports your claim. Include REASONING: Explain WHY you selected that evidence to support your claim.   Hint attached.

4fe+3o2⟶2fe2o3 how many grams of Fe2O3 will be produced from 37.5 grams of iron? show work.

4. True or False (1) Chlorine demand is the difference between total chlorine and free chlorine (2) In raw wastewater samples, most of nitrogen is in the form of nitrate. (3) If 10 mg/L of NH3-N is converted to nitrate, the nitrate concentration is 10 mg/L as N. (4) Free chlorine consists of hypochlorous acid and hypochlorite. (5) Chloramines is a weaker disinfectant than free chlorine. (6) Na2HPO4 contributes to the orthophosphates. (7) For phosphorus analysis, the purpose of the autoclave is to kill the phosphorus bacteria which interferes colorimetric analysis. (8) Chloride is an effective disinfectant for water and wastewater treatment. (9) "Crown" corrosion is caused by the corrosive action of H₂SO4. (10) Breakpoint chlorination can be used for removal of ammonia.

Consider the following reaction: Fe2+ (aq) + 2Cl¯ (aq) →Fe(s) + Cl₂ (g) To make this reaction occur with the excess amounts of both reactants, 8.0 A of electric current flow into the reaction for 5.0 minutes. How many grams of Fe would be produced at this condition? 0.43 g 0.69 g 1.4 g 0.27 g O 2.1 g

The extraction of aluminum metal from the aluminum hydroxide found in bauxite by the Hall-Héroult process is one of the most remarkable success stories of 19th century chemistry, turning aluminum from a rare and precious metal into the cheap commodity it is today. In the first step, aluminum hydroxide reacts to form alumina Al2O3  and water:   2Al(OH)3(s) + Al2O3(s) ->  3H2O(g) In the second step, alumina Al2O3  and carbon react to form aluminum and carbon dioxide:   2Al2O3(s) +  3C(s) + 4Al(s) ->  3CO2(g) Suppose the yield of the first step is 74.%  and the yield of the second step is  76.% . Calculate the mass of aluminum hydroxide required to make  4.0kg  of aluminum.   Be sure your answer has a unit symbol, if needed, and is rounded to the correct number of significant digits.

5. Consider the following equation: 2C2H6 + O2 -> 4CO2 + 6H2O When .004 moles of C2H6 are burned the number of moles of CO2 produced will be?

The reduction of iron(III) oxide to iron during steel-making can be summarized by this sequence of reactions: 20(s) +0, (g) =2 CO (g) K, Fe,0, (s) +3 CO (g) =2 Fe (1) +3 CO, (g) K2 The net reaction is: 2 Fe,O, (s) +6C (s) +30, (g)=4 Fe (1) +6CO, (3) K Write an equation that gives the overall equilibrium constant K in terms of the equilibrium constants K, and K,. If you need to include any physical constants, be sure you use their standard symbols, which you'll find in the ALEKS Calculator. K = 믐 Submit Assign Continue MacBook Air F7 000 吕口 000 FA F5

How to balance chemical equations. Please explain the equation below. What strategy is used to balance it? 2Na(s) + F2(g) → 2NaF(s)

The extraction of aluminum metal from the aluminum hydroxide found in bauxite by the Hall-Héroult process is one of the most remarkable success stories of 19th century chemistry, turning aluminum from a rare and precious metal into the cheap commodity it is today. In the first step, aluminum hydroxide reacts to form alumina (Al,0,) and water: 2Al(OH), (s) Al,0; (s) + 3 H,0 (g) - In the second step, alumina (Al,0,) and carbon react to form aluminum and carbon dioxide: 2Al,0; (s) + 3C(s) → 4Al(s) + 3 CO, (g) Suppose the yield of the first step is 82.% and the yield of the second step is 69.%. Calculate the mass of aluminum hydroxide required to make 10.0 kg of aluminum. Be sure your answer has a unit symbol, if needed, and is rounded to the correct number of significant digits. x10

The chart shows average CO2 emissions for fossil fuel vehicles (gasoline, diesel, and hybrid gas‑electric), as well as electric vehicles. The ordinate is mg CO2 per mile driven per pound mass of the vehicle (called curb weight). For electric vehicles, CO2 emission varies in U.S. states because of the mix of fuels used to generate electricity. If electricity came entirely from solar power, there would be little CO2 associated with its production. California has the lowest CO2 emission for producing electricity and Ohio has the highest because it depends heavily on coal‑fired power plants. The chart does not include CO2 emission from manufacturing vehicles. When normalized for distance driven by each kind of vehicle before it is scrapped, CO2 emission associated with manufacturing electric vehicles is estimated to be 25–75% greater than CO2 emission associated with manufacturing gasoline and diesel vehicles. If manufacturing were included, CO2 emission associated with electric vehicles…

Hi! Can you be so kind to help me do #5,#6,#8 and #10. Thanks!

Ammonification is the process by which A B C ammonia is released during the decomposition of nitrogen-containing organic compounds ammonium is converted to nitrite and nitrate in soils nitrate from soil is transformed to gaseous nitrogen compounds such as NO, N₂O, and N₂ D gaseous nitrogen is fixed to yield ammonia 4

* What amount (in mol) and what mass (in kg) of carbon dioxide are produced when 20 gallons (approximately 2.0 x 10' kg) of octane (C3H18) is combusted? C3H18(1) +O2(g) CO2(g) + H;O(1) A: 1.4 x 10°; 62

What is number 1-B

When potassium metal is placed in water, a large amount of energy is released as potassium hydroxide and hydrogen gas are produced in the reaction 2K(s) + 2H2O(l) → 2KOH(aq) + H2(g). Your lab partner says this is a redox reaction and a combustion reaction. Do you agree? Defend your answer by explaining whether or not it meets the requirements of each type of reaction.

Consider the microbial conversion of glucose to L-glutamic acid, as shown below. Assume that initially the bioreactor contains 200 kg of glucose, 15 kg of ammonia and 54 kg of O2. C6H1206 + NH3 +1.5 O2 →C5H9NO4+ CO2 + 3H2O glucose ammonia glutamic acid a) Which reactant is limiting? b) What is the percentage excess of the other reactants? c) If the reaction proceeds to completion, how much of the excess reactants will be left; how much L-glutamic acid will be formed; and what is the extent of reaction ? d) If the reaction proceeds to a point where the conversion of the limiting reactant is 33%, how much of each reactant and product is present at the end, and what is the extent of reaction E ? e) If the reaction proceeds to a point where 35 kg of O2 is left, what is the fractional conversion of glucose? What is the fractional conversion of O2? What is the extent of reaction E ?

1. LIAIH4, Et₂O 2. H₂O

Describe how the following changes are brought about: (i) Pig iron into steel. (ii) Zinc oxide into metallic zinc. (iii) Impure titanium into pure titanium.