Compute the theoretical oxygen demand of 34 mg/L of bacterial cell C5H7NO2. Assume the following reactions apply. C5H7NO2 + 502 5CO2 + 2H20 + NH3 ---- NH3 + 202 ---- NO3 + H + H2O
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- The equilibrium constant for the reaction below is 1.8 x 1019 at 298K. What is the value of the standard cell potential for this reaction? Nij + Hg²CI?«) 2Hg) + 2Cl (aq) + Ni2+, (aq) Determine the cell potential for this reaction. O 0.57 J/C O 1.02 J/C O 0.24 J/CNaOH (aq) + HCI (aq) NACI (aq) + H2O (1) Volume of 1.00M HCI (mL) 45.0 Volume of 1.00 M NAOH (mL) 50.0 Initial Temperature ("C) 22.1 Final Temperature (C) 31.6 la) Calculate the moles of HCI used in the reaction. Moles of HCI = mol (b) Calculate the moles of NaOH used in the reaction. Moles NaOH= mol (c) Which reactant is the Limiting Reactant, HCl or NaOH? Limiting Reactant = (d) Is this acid-base neutralization reaction exothermic or endothermic? NOTE: DO Include the correct number of significant figures or you will be marked wrong and DO NOT include units in your answer.When chlorine (Cl2) gas is added to water during the disinfection of drinking water, it hydrolyzes with the water to form hypochlorous acid (HOCI). The disinfection power of the acid HOCI is 88 times better than its conjugate base, OCI". The pKa for HOCI is 7.5. Because the acidic form is a much better disinfectant, you want to maintain 89% of the total molar concentration in this form. What minimum pH should you target? Correct answer 6.6
- Q3: A: What mass of AgNO3 is needed to convert 3.46g of Na2CO3 to Ag2CO3, and calculate the mass of Ag2CO3 will be formed? Discuss your results. 2A9NO3(aq) +N22CO3(aq) → Ag2CO3(e) + 2NaNo3(aq)A drinking water treatment plant wants to compare the efficacy of three different solid coagulants, Alum [Al(OH)3(s)], Lime (CaCO3(s)), and Ferric Chloride (FeCl3(s)), for removing the phosphate (PO43-) level to 1 mg/L. The following are the equilibrium reactions [and the respective equilibrium constants (or solubility products, Ksp)] that result in phosphate removalfor each solid, the second reaction being more relevant in each case: Alum: Al(OH)3(s) ↔ Al3+ + 3OH- AlPO4(s) ↔ Al3+ + PO43- Ksp = 9.84 x 10-21 Lime: CaCO3(s) ↔ Ca2+ + CO32- Ca3(PO4)2(s) ↔ Ca2+ + PO43- Ksp = 1 x10-27 Ferric Chloride: FeCl3 (s) ↔ Fe3+ + 3Cl- Fe(PO4)(s) ↔ Fe3+ + PO43- Ksp = 1x10-26.4 What concentrations of Fe 3+, Al3+, and Ca2+ will be needed to maintain a phosphate concentration of 1 mg/L? What would be the best choice of solid coagulant for the Drinking Water Treatment Plant?…Environmental Engineering, environmental chemistry question: Hydrogen sulfide (H2S) is an odorous gas that can be stripped from solution. The reaction is: H2S<<<>>>H+ + HS- The equilibrium constant, Ka1 = 0.86 x 10-7 Find the fraction of hydrogen sulfide in H2S form at pH 6 and pH 8.
- (a) Draw the appropriate curved arrows and products for each set of reactants undergoing a coordination step. Identify each reactant species as either a Lewis acid or a Lewis base. (b) Use curved arrow notation to show each product undergoing heterolysis to regenerate reactants. (i) NH, (ii) (ii) H, C. + AICI3 H,O + BF3 H3C6. Ammonia, NH3, is a base and will readily accept a proton in accordance with the following reaction NHxaq) + H,O=NH,+ + OH- (a) Calculate the equilibrium constant, K, for this reaction at 25°C. (b) If, at some time, pH reaction at equilibrium? If not, in which direction is the reaction going? 9.0, [NH3} = 10-5 M, and [NH,*} 10-6 М, is the4 UEME1233 MANUFACTURING TECHNOLOGY I Hot working is a process commonly seen in the production floor that usually involved heating furnaces. Explain one reason of hot working and justify the types of heat-treating furnaces. Q1. (а) (Word limit: ~150) (b) Discuss the importance of understanding in crystal structure of metal and why different crystal structures exhibit different strengths and ductility. (Word limit: ~150)
- Q.1: For the following reaction : K3PO4 (aq) + Al(NO3)3 (aq) ? AIPO4 (s) + KNO3 (aq) a- Write the balance molecular equation, b- Write the complete ionic equation, C- Write the net ionic equation.The most important buffer system in water is the carbon dioxide system of acid/base reactions. CO2(g) → CO2(aq) + H2O(1) → *H2CO3 +→ H* + HCO3 2H* + CO32- A sample of water has a pH of 5.0 the concentration of HCO3 is 122 mg L-1and the CO3- concentration is 60.0 mg L-1. What is the approximate alkalinity (ALK) in the water as CaCO3? Assume there is no exchange between the solution and the atmosphere and the temperature is 25°C. ALK= [HCO3] + 2[CO3²]]A water has the following analysis (mg/L as ion or compound): Na+ 20 mg/L 40 mg/L K 30 mg/L 67 mg/L Ca²+ 15 mg/L 0 mg/L Mg2+ 20 mg/L 5 mg/L 2 mg/L 10 mg/L Sr²+ CI HCO3 2- CO3²- SO₂²- NO3 Atomic weight of Na = 23, K = 39.10, Ca = 40.08, Mg = 24.31, Sr= 87.62, Cl = 35.45, H = 1, C = 12, 0 = 16, S = 32.07, and N = 14) What is the total hardness in mg/L as CaCO3? What is the carbonate hardness in mg/L as CaCO3? A/ What is the noncarbonate hardness in mg/L as CaCO3? A/