# environmental chemistry homework help

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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: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
• Q16:1. A military base is contaminated with a plume of dinitrophenyl acetate (DNPA) that has leaked from an underground storage tank. In order to understand the degradation potential, a colleague of yours measured the change in DNPA concentration over time in pH 5.0 and pH 8.5 solutions at 22.5 °C and for a temperature range of 17.7 to 30 °C (only for pH 5.0 solution, shown next to part d). (a) Determine the molecular formula and calculate the molecular weight of DNPA. Show ALL of your work for full credit.See Answer
• Q17:(b) Determine the rate coefficients (kh) of the hydrolysis reaction at 22.5 °C for pH 5.0 and pH 8.5 by graphing the data. What is the reaction order and quantity of the two rate coefficients? Show all graphs and fit equationsSee Answer
• Q18:(c) The pK of DNPA is 2.5. What is the fraction of DNPA in the protonated and deprotonated forms at pH 3.0?See Answer
• Q19:(d) It has been observed that temperature has an effect on the reaction rate. Using the data below, calculate the Arrhenius activation energy (No; in units of kJ mol ‘) for the hydrolysis of DNPA at pH 5.0. Keep in mind that the Arrhenius equation can be written as Ink —— ——° — + cSee Answer
• Q20:(e) Without any information about DNPA, your colleague asks you what other reaction pathways might be possible to degrade ONPA if the contaminated groundwater eventually mixes with a nearby creek. To start the brainstorming process, in words, list some other possibilities of reactions in the environment and explain how these might degrade DNPA.See Answer

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