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Q1:3.10 What would be the saturation concentration (mole/L) of oxygen (O₂) in a river in winter when the air temperature is 0°C if the Henry's law constant at this temperature is 2.28 x 10³ mole/L-atm? What would the answer be in units of mg/L?See Answer
Q2:3.13 The Henry's law constant for H₂S is 0.1 mole/ L-atm, and H₂S (aq) HS + H+ where K₁ = 10-7. If you bubble pure H₂S gas into a beaker of water, what is the concentration of HS at a pH of 5 in (a) moles/L, (b) mg/L, and (c) ppmm?See Answer
Q3:3.14 Determine the equilibrium pH of aqueous solutions of the following strong acids or bases: (a) 15 mg/L of HSO4, (b) 10 mM NaOH, and (c) 2,500 Hg/L of HNO3.See Answer
Q4:3.31 A first-order reaction that results in the destruc- tion of a pollutant has a rate constant of 0.1/day. (a) How many days will it take for 90 percent of the chem- ical to be destroyed? (b) How long will it take for 99 per- cent of the chemical to be destroyed? (c) How long will it take for 99.9 percent of the chemical to be destroyed?See Answer
Q5:3.33 Assume PO is removed from municipal wastewater through precipitation with Fe³+ according to the following reaction: PO4 + Fe³+ →FePO4(s). The rate law for this reaction is d[PO³ = -k[Fe³+ ][PO³] dtSee Answer
Q6:Burning nitrobenzene NO₂ Nitrobenzene (NB) is an organic compound with the chemical formula C6 Hs NO2. It is produced on a large scale from benzene as a precursor to aniline. Nitrobenzene is highly toxic (Threshold Limit Value 5 mg/m³) and readily absorbed through the skin. A tank contains 3076.5 kg of residual NB, which must be destroyed by incineration, thus converted into harmless compounds (CO2, H₂ O, NO2). However, a malfunction of the burner, because the excess air did not reach the set point (150%), resulted into incomplete combustion and formation of undesired side products (CO). Once the incident analyzed, we were aware that the actual excess air was only 20%. Then, the conversion was only 90%. In addition, the ratio between CO₂ and CO was 4 to 1 (total combustion against partial combustion)./nTotal: Partial: C6 Hs NO2 + 29/4 02 C6 Hs NO2 + 17/4 02 → 6CO₂ + NO2 + 5/2H₂O 6 CO + NO2 + 5/2 H₂O Taking into account the given TLV, did the flue gas emitted put in danger people? Note: we assume that the end product for nitrogen is NO2See Answer
Q7:Why is my teacher having me do this project?? A. To practice empirical/molecular formula calculations, stoichiometry, and gas law calculations. (M3, M4, M5) B. To practice writing combustion reactions. (Outcome 4.3) C. To learn a little about combustion, flammability, flame temperature, and molecular structureSee Answer
Q8:Part A: Empirical and Molecular Formulas (Outcomes 3.1, 3.2, 3.3) From the combustion analysis data given for your sample determine the empirical formula. Using the molar mass, determine the molecular formula. ALL COMPOUNDS ARE HYDROCARBONS (NO OXYGEN) • Confirm your molecular formula by researching using the boiling point and melting point as your guide.See Answer
Q9:Part B: Nomenclature and Molecular Structure (S2, S3) • What is the formal / IUPAC name for your compound? Does your compound also go by any other common names? • Draw a structure of your compound that shows the bonding. There is a cool online tool called MolView that you can use. Include the image of your compound in your report. Have fun with this site!See Answer
Q10:Part C: Combustion Reactions (Outcome 4.3) Watch this video and then explain the difference between complete and incomplete combustion. Write the balanced reaction for BOTH the complete AND the incomplete combustion of your fuel. •See Answer
Q11:Part D: Gases (Outcomes BI 4, 5.1, 5.2, 5.3, BI 1, S4) Determine the total moles of gases formed from the complete combustion of 1.0 kilogram of your fuel. Assume that water is in the gas phase. o Calculate the mole fraction of each gas produced and their partial pressures (in atm) if the total pressure is 760. mm Hg. If this combustion happens at STP, what volume will these gases occupy? o Is this volume accurate? As this gas is combusting will it really stay at standard temperature? What is the flame temperature of your compound? (Research this!) *Note: if you cannot find this temperature, use 3000.ºC. Calculate the final volume of gas produced from 1.0 kg of fuel using the flame temperature. o Think to the gas laws in Module 5. Assume constant pressure.See Answer
Q12:Part E: Research (Outcomes S2 and S3) What is the flash point of your compound? What does this mean? Is your compound considered flammable or combustible? What is the difference between these properties? How should your compound be stored safely? What kind of container should it be in? Should it be exposed to air? Should it be kept at a certain temperature? Design this for me. Find the Hazard Symbol Diamond for your fuel. What do these numbers and colors mean in this symbol? What is your compound commonly used for-engineering or otherwise?See Answer
Q13:Part F: Citations (Outcome S5) Cite ALL your sources. You can hyperlink them, but I also need the citations. This should be a section at the end of your document.See Answer
Q14:Instructions: TOPIC OF ESSAY: CHEMISTRY in HEALTH-CARE, CLIMATE CHANGE and ENVIRONMENT PROTECTION. Write an essay based on the topic above. Word count - 500 words Double spacedSee Answer
Q15:6-1. The following mineral analysis was reported for a water sample taken from Well No. 1 at the Eastwood Manor Subdivision near McHenry, Illinois (Woller and Sanderson, 1976a). Well No. 1, Lab No. 02694, November 9, 1971 Iron 0.2 Silica (SiO2) 20.0 Manganese 0.0 Fluoride 0.35 Ammonium 0.5 Boron 0.1 Sodium 4.7 Nitrate 0.0 Potassium 0.9 Chloride 4.5 Calcium 67.2 Sulfate 29.0 Magnesium 40.0 Alkalinity 284.0 as CaCO, Barium 0.5 pH 7.6 units Note: All reported as "mg/L as the ion" unless stated otherwise. Determine the total, carbonate, and noncarbonate hardness in mg/L as CaCO, using the predominant polyvalent cation definition in Section 6- 3. Answers: TH=332.8 mg/L as CaCO3 CH= 284.0 mg/L as CaCO, NCH 48.8 mg/L as CaCO, Last mo mal Jan 25See Answer
Q16:"Not in mg/L.. 6-13. Determine the lime and soda ash dose, in mg/L as CaCO3, to soften the following water to a final hardness of 80.0 mg/L as CaCO3. The ion concentrations reported below are all mg/L as CaCO3. Ca² = 120.0 Mg2+= 30.0 Last m mal Jan 25 HCO3 = 70.0 CO₂ = 10.0 Answers: Total lime addition = 100 mg/L as CaCO, Total soda ash addition = 40 mg/L as CaCO,See Answer
Q17:6-15. Determine the lime and soda ash dose, in mg/L as CaO and Na2CO3, to soften the following water to a final hardness of 80.0 mg/L as CaCO3. The ion concentrations reported below are all mg/L as CaCO3. Assume the lime is 90 percent pure and the soda ash is 97 percent pure. Ca2+-210.0 Mg2+= 23.0 HCO=165.0 CO₂ = 5.0 Answers: Total lime addition = 118 mg/L as CaO Total soda ash addition = 31 mg/L as Na₂CO,See Answer
Q18:CO₂ = 7.0 6-19. What amount of lime and/or soda ash, in mg/L as CaCO3, is required to soften the Village of Zap's water to 80.0 mg/L hardness as CaCO3? Last modified Jan 25, 2024 learnandcare. Compound Concentration, mg/L as CaCO3 CO₂ 44.2 87.4 Mg2+ 96.3 HCO₂ 204.6 so 73.8See Answer
Q19:6-30. What is the volume required for a rapid-mix basin that is to be used to treat 0.05 m³/s of water if the detention time is 10 seconds? Answer: 0.5 m³See Answer
Q20:the detention time of each tank? 6-33. Determine the power input required for the tank designed in Problem 6- 30 if the water temperature is 20°C and the velocity gradient is 700 s. Answer: 245.49 or 250 W or 0.25 kWSee Answer

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