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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: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
Q6: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
Q7: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
Q8: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
Q9: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
Q10: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
Q11:"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
Q12: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
Q13: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
Q14:6-40. Your boss has assigned you the job of designing a rapid-mix tank for the new water treatment plant for the town of Waffle. The design flow rate is 0.050 m³/s. The average water temperature is 8°C. The following design assumptions for a rapid-mix tank have been made: 1. Number of tanks = 1 (with 1 backup) 2. Tank configuration: circular with liquid depth = 1.0 m 3. Detention time = 5 s 4. Velocity gradient 750 s¹ 5. Impeller type: turbine, 6 flat blades, Np=3.6 6. Available impeller diameters: 0.25, 0.50, and 1.0 m 7. Assume B=H Design the rapid-mix system by providing the following: 1. Water power input in kW 2. Tank dimensions in m 3. Diameter of the impeller in m 4. Rotational speed of impeller in rpm Continuing n of the tmont Jan 25, 2024 learnandcareSee Answer
Q15:1. (4 pts total) The mass of Earth's atmosphere is approximately 5.27 x 10¹8 kg or 5.27 x 106 gigatonnes (Gt). Given that the concentration of CO₂ in the atmosphere has increased from 280 ppm in the 18th century to approximately 410 ppm, today, estimate the increase in the mass of carbon in the atmosphere over this time period. (Hint: start by converting the mass of the atmosphere to total moles of air in the atmosphere).See Answer
Q16:2. (4 pts total) Ammonia (NH3), nitrous oxide (N₂O) and methane (CH4) comprise 1 x 10-8, 3 x 10-5 and 7 x 10-5 % by mass of the Earth's atmosphere, respectively. If these compounds are removed from the atmosphere at rates of 5 x 10¹0, 1 x 10¹0 and 4 x 10¹1 kg yr¹, respectively, what are the lifetimes of NH3, N2O and CH4 in the atmosphere? What do your results imply about the spatial distribution of each of these compounds (in other words: are their concentrations likely to be uniform or variable over city, state, or the continent)? Why?See Answer
Q17:3. (6 pts total) The average lifetime (i.e. e-folding time) for CFC-12 molecules to be lost in the atmosphere by photolysis is 116 years. Assuming no emissions after 2003 due to implementation of the Montreal Protocol, calculate the amount of CFC-12 that should be in the atmosphere (i) now, (ii) in 2050, and (iii) in 2200. The amount present in 2003 was 540 ppt (parts per trillion). The actual amount in the atmosphere now is about 500 ppt. Why might your answer be different from the actual amount? (Hint: you will need to use the integrated form of the first order rate law to answer this question).See Answer
Q18:4. (10 pts total) Use the typical vertical profile of ozone number concentration (molecules/cm³) to answer the following questions. z, km 40 25 10 012345 O3 profile piecewise linear approximation 03, 10¹2 molecules cm¹³3 a. (5 pts) Calculate the mixing ratio of O3 at sea level (z = 0 km, P = 101,300 Pa, T = 300 K) and 25 km (P = 3500 Pa, T = 220 K). Why does the difference in mixing ratios at 0 km and 25 km appear larger than the difference in number concentrations? b. (2 pts) The total number of O3 molecules in the atmosphere per unit area (for example, 1 cm²) is called the "O3 column concentration" and determines the efficiency with which the O3 layer prevents UV radiation from reaching the Earth's surface. Estimate the O3 column (i.e., molecules per cm²) in the above profile by approximating the profile with the "piecewise linear function" shown as the thin solid line (Hint: recall that the area of a triangle is 2*base*height). c. (3 pts) To illustrate how thin the stratospheric ozone layer actually is, imagine that all of the O3 in the atmospheric column you calculated in part (b) were brought to sea level as aSee Answer
Q19:5. (12 pts total) Answer the following questions using the information below: Reaction (1): C1+03 → CIO + O2 Reaction (2): 0+ CIO → C1 + 02 Reaction (3): Cl + CH4 → HCl + CH3 Reaction (4): 0+03 → 02 +02 kı = 9.1x10-¹2 cm³ molecule-¹ s-¹ k₂= 4.1x10-¹1 cm³ molecule-¹ s-¹ k3= 2.2x10-¹4 cm³ molecule-¹ s-¹ k4 = 8.5x10-¹6 cm³ molecule-¹ s-¹ Mixing ratios (i.e., Xz, where z is Cl, O3, O, CIO or CH4) by volume at 30 km altitude: Cl=1.7x10-¹3 (i.c., 0.17 ppt or parts-per-trillion), O3-8.3×10-6, 0-8.9×10-¹¹, CIO=1.9×10-10, CH4=6.7x10-7. The total pressure at 30 km is 1.13% of its value at the ground, and the temperature is 224 K. a. (2 pts) Re-arrange the ideal gas law to express concentration in terms of pressure and temperature. Use this expression to calculate the concentration of air at 30 km altitude, in units of the number of air molecules per cubic centimeter of air. (The answer is 3.7×10¹7 molecules/cm³) b. (2 pts) Calculate the concentrations of Cl, O3, O, CIO and CH4. c. (2 pts) Reaction (2) is the rate-determining step of the chlorine catalytic cycle. At what rate is odd oxygen destroyed by chlorine radicals? (Hint: to answer this, remember that "odd oxygen destruction" includes loss of both O and O3) d. (3 pts) What is the lifetime of odd oxygen from loss in the fourth reaction of the Chapman scheme (i.e., Reaction 4, above)? What is the lifetime via chlorine catalysis (use your answer from (c))? Based on your calculation, is chlorine catalysis important for ozone loss relative to the rate of loss via Chapman chemistry? e. (3 pts) Assuming that the only important chemistry involving chlorine-containing radicals is that shown above, calculate how many odd oxygen molecules are destroyed by a single Cl atom before that chlorine atom is converted to HCl. (Hint: To do this, try comparing the lifetime for loss of Cl atoms via reaction with ozone to that for loss via reaction with CH4.)See Answer
Q20:The project requires to build a carbon capture and utilisation plant to capture the CO2 produced in the above power plant and convert the captured CO₂ to CO using renewable hydrogen. Calcium looping technology will be used, although a broad review of carbon capture technologies will be included in the report. The project is to produce a concentrated stream of CO₂ (over 95 Vol.%) which will then be used to production CO through hydrogenation. The design must ensure that the health, safety and environmental (HSE) risks are as low as reasonably practical (ALARP) and meet all current and reasonably foreseeable safety and environmental legislation. In addition, the process control scheme should ensure that the plant operates normally under full automatic control, and provide sufficient information for its performance to be monitored and optimised.See Answer

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