Chlorinated solvents such as carbon tetrachloride (CCl4) can be degraded in a process called reductive dechlorination where Cl atoms are removed and replaced with H atoms. For example: CCl4 + H+ +2e ⇒ CHCl3 +CI-E⁰=0.67 V In the process of in situ bioremediation an electron donor such as acetate (CH3COO-) is typically added and is oxidized to provide the electrons for the reduction of CCI4. In groundwater devoid of oxygen, nitrate typically serves as the electron acceptor. Answer the questions below using data from Appendix A and that provided above. i) Is it possible that CCl4 could serve as an electron acceptor for acetate? ii) Which electron acceptor, CCl4 or NO3, would be thermodynamically preferred? iii) What do the results in i and ii imply for remediation in an aquifer containing nitrate? (provide a qualitative answer)

Chlorinated solvents such as carbon tetrachloride (CCl4) can be degraded in a process called reductive dechlorination where Cl atoms are removed and replaced with H atoms. For example: CCl4 + H+ +2e ⇒ CHCl3 +CI-E⁰=0.67 V In the process of in situ bioremediation an electron donor such as acetate (CH3COO-) is typically added and is oxidized to provide the electrons for the reduction of CCI4. In groundwater devoid of oxygen, nitrate typically serves as the electron acceptor. Answer the questions below using data from Appendix A and that provided above. i) Is it possible that CCl4 could serve as an electron acceptor for acetate? ii) Which electron acceptor, CCl4 or NO3, would be thermodynamically preferred? iii) What do the results in i and ii imply for remediation in an aquifer containing nitrate? (provide a qualitative answer)

Chemistry

10th Edition

ISBN:9781305957404

Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Chapter1: Chemical Foundations

Section: Chapter Questions

Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...

See similar textbooks

Similar questions

Question 1 Identify the organic class to which the compound belongs based on the functional groups present. [Hint - Organic class such as Ester, Ether, Carboxylic acid, Aldehyde, Ketone, Amine, Amide, Alcohols, if more than on Functional group present identify both, left then right separated by;] CH 3 Paragraph Previous Page B I Next Page A/ E✓ E 11 GO + v 11. Page 1 of 30
Calculate the solubility at 25 °C of PbCO3 in pure water and in a 0.0120M Pb(NO3), solution. You'll find Kp data in the ALEKS Data tab. sp Round both of your answers to 2 significant digits. solubility in pure water: solubility in 0.0120 M Pb(NO3)2 solution: 170 170 ☐x10 X 0x0 00
Calculate the solubility at 25 °C of Zn(OH), in pure water and in a 0.0190M ZnSO solution. You'll find Kp data in the ALEKS Data tab sp Round both of your answers to 2 significant digits. solubility in pure water: solubility in 0.0190 M ZnSO4 solution: 0 -/- 0 -/-/- 00 10 X OXO 5 00
Ksp for BaCrO4 is 1.17x10^-10
8. Assume that the following exchangeable cations are present in a 25 gram sample of a soil Cation Са Al wt (g) 0.120 0.072 Mg K 0.036 0.234 H NH4* 0.007 0.054 a) If it assumed that no other cations are present in the exchange complex, what is the CEC of the soil? b) Calculate the base saturation (%) and hydrogen saturation (%)
Lable the reactios as single-displacement, double displacement, synthesis decomposition HCl(aq)+NaHCO3(aq)-->Co2(g)+H20(l) AgNO3(aq)+HCl(aq)-->AgCl(s)+HNO3(aq) HFe(s)+302(g)-->2Fe2)3(s)
A highly acidic (pH< 0.5) industrial wastewater has an initial AlP" concentration of 10 ppm. An engineer decides that strong base should be added to the wastewater in order to raise the pH so that most of the aluminum will precipitate and be removed from solution. The pertinent solubility reaction from Appendix A of our text is: Al(OH)3 (s) → Al* + 30H¯ with pK, = 32.9 a. What is the lowest pH needed to precipitate all but 50 ppb of the aluminum from the wastewater? Assume equilibrium conditions can be achieved. b. Suppose the engineer decides that the pH should be raised to 7. What equilibrium concentration of aluminum would be left in solution? Report your answer in ppb and moles per liter.
Please help using the information below calculate the limiting reagent and the theoretical yield
Calculate the solubility at 25 °C of Co(OH)₂ in pure water and in a 0.0140 M CoCl₂ solution. You'll find Kp data in the ALEKS Data tab. Round both of your answers to 2 significant digits. solubility in pure water: 0-/-/- solubility in 0.0140 M CoCl₂ solution: 0 0 x10 X OXO 0/0
A monoprotic weak acid, HA, dissociates in water according to the reaction HA(aq) =H*(aq) + A (aq) The equilibrium concentrations of the reactants and products are (HA] = 0.240 M, [H*] = 4.00 x 10 M, and = 4.00 x 10- M. Calculate the value of pK, for the acid HA. %3D %3D [A] pK, =
The compound you will be investigating in this experiment is the ionic salt barium nitrate, Ba(NO3)2. (a) Write the balanced equilibrium reaction for the dissolution of barium nitrate in a satu- rated solution and the expression for the solubility product, Ksp. (b) Write the mathematical relationship between the molar solubility of barium nitrate and the concentrations of the barium ions in the saturated solution [Ba2+]eq and nitrate ions in the saturated solution [NO3–]eq. (c) Write an equation that relates the molar solubility of barium nitrate and the solubility product Ksp, similar to how Equation 3 in the Background was written for sodium chloride. (d) Consider dissolving the barium nitrate in nitric acid HNO3, a strong acid (it reacts completely with water to form hydronium and nitrate ions), instead of water. Does the nitric acid influence the barium nitrate’s solubility equilibrium? If so, how, and will this cause more or less barium nitrate to dissolve in the…
The following chemical reaction was performed in a laboratory to produce copper(1) iodide for a biochemistry investigation. Experimenters started with excess copper(II) chloride, but a limited amount (855 mg) of potassium iodide. 2CuCl2 + 4KI→2Cul+ 4KCl + 1₂ 1) Calculate the theoretical yield mass of copper(1) iodide, in milligrams. [Seleccionar] 2) In the lab, they were able to experimentally produce 326 mg of copper(1) iodide. What is the percent yield? [Seleccionar ]