Calculate the overall reduction potential for the following couples. Write out both half reactions and the overall reaction, Use electrons, water, and protons to balance the reaction. Indicate which molecule is the electron donor and which molecule is the electron acceptor in the overall reaction. The T button allows you to add superscripts and subscripts. Use--> for arrows. NAD/NADH E,-0.32V NO2/NO E +0.36V

Calculate the overall reduction potential for the following couples. Write out both half reactions and the overall reaction, Use electrons, water, and protons to balance the reaction. Indicate which molecule is the electron donor and which molecule is the electron acceptor in the overall reaction. The T button allows you to add superscripts and subscripts. Use--> for arrows. NAD/NADH E,-0.32V NO2/NO E +0.36V

Fundamentals Of Analytical Chemistry

9th Edition

ISBN:9781285640686

Author:Skoog

Publisher:Skoog

Chapter22: Bulk Electrolysis: Electrogravimetry And Coulometry

Section: Chapter Questions

Problem 22.20QAP

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Below are the reduction half reactions for chemolithoautotrophic nitrification, where ammonia is a source of electrons and energy and oxygen is the terminal electron acceptor. NO2- + 6e- -> NH4+ (E0 = +0.34 volts) O2 + 4e- -> 2H2O (E0 = +0.82 volts) If you balance and combine the reactions so that 293 moles of NH4+are oxidized to NO2-, how many moles of electrons will be transferred from Nitrogen to Oxygen?
Given the standard reduction potentials (Eo’) for ubiquinone (Q) and NADP+provided below, consider the following questions.Q + 2H+ + 2e- ---> QH2 Eo’ = 0.04 VNADP+ + H+ + 2e- ---> NADPH Eo’ = -0.32 V - Calculate the standard ΔEo’ for the oxidation of NADPH by Q. From the reactantsin your derived redox reaction, indicate the oxidant and reductant.- Calculate the standard free energy of the redox reaction in part (a) and indicate if thereaction is exergonic or endergonic.
What is the purpose of immersing the electrode in a saturated KCl solution? Is it proper to store the electrode in deionized water? Why or why not? Explain clearly and thoroughly.
please show the given and required as well as the half-reactions for a more detailed format.
Consider the reaction of pyruvate with NADH and the standard reduction potentials, ?′°,E′°, of pyruvate and NAD+. Redox pair E'°, V pyruvate/lactate –0.19 NAD+/NADH –0.32 pyruvate+NADH↽−−⇀lactate+NAD+ Assuming that the concentrations of each reactant and product are 1 M and that the reaction is performed at pH 7 and 25 °C, determine the Δ?′°Δ⁢E′° for the reaction.
Use the standard reduction potentials located in the 'Tables' linked above to calculate the equilibrium constant for the reaction: Hint: Carry at least 5 significant figures during intermediate calculations to avoid round off error when taking the antilogarithm. https://cxp.cengage.com/contentservice/assets/owms01h/references/chemtables/gen_chem/eo.html
5. discuss your generalizations and realization after learning about standard reduction potential please do not just copy from google, i will upvote. thx
A cell consisting of a saturated calomel electrode and a lead ion electrode developed a potential of -0.3257 V when immersed in a 60.00 mL lead solution of unknown concentration. A 10.00 mL addition of 0.02500 M lead standard solution caused the reduction potential to shift to -.2897 V. Calculate the molar concentration (in units mM) of lead in the sample. Please make sure to perform necessary calculations to have a final answer in mM.
2 Two nitroimidazole drugs, misonidazole and tinidazole have single-electron reduction potentials of -0.389 V and -0.464 V respectively: Misonidazole + e- ➝ Misonidazole·- E0 = -0.389 V Tinidazole + e- ➝ Tinidazole·- E0 = -0.464 V The reduction potential of the NADH/NAD couple is -0.324 V, and the reduction potential of the ferrodoxin couple is -0.460 V: NAD+ + e- ➝ NADH E0 = -0.324 V [Ferrodoxin]3+ + e- ➝ [Ferrodoxin]2+ E0 = -0.460 V Explain which, if any, of misonidazole and tinidazole will be selectively reduced in protozoa over mammalian cells. In your answer you should calculate any reduction potentials you need.
In a polarographic experiment of a 60 mL of 0.08 M Cu2+solution, a limitingcurrent was left on for 15 minutes. If the average current during the time of theexperiment is 6.0 μA, what fraction of the copper is removed from the solution? TheFaraday constant is 96485 C/mol of electron.
3) Construct two electrochemical cells such that the EMF of the cells are less than +0.513 V. a. Before doing the simulation, predict the cells and explain. Justify using the Nernst equation. b. Provide the shorthand notation and EMF for each of the electrochemical cells that you construct.
Use standard reduction potentials to calculate the equilibrium constant for the reaction:Hg2+(aq) + 2Ag(s)---> Hg(l) + 2Ag+(aq)Hint: Carry at least 5 significant figures during intermediate calculations to avoid round off error when taking the antilogarithm.Equilibrium constant: ____G° for this reaction would be (greater, less) than zero.