Given the following standard reduction table:REDUCTION REACTIONE", VNAD + H'+2eNADH-0.32Pyruvate + 2H" + 2eLactate-0.19Fumarate + 2H" + 2eSuccinate-0.03Oxaloacetate + 2H + 2eMalate0.17while the STRONGEST REDUCING agent1. Based on the listed half-reactions, the STRONGEST OXIDIZING agent isis2. Consider the overall reaction, where a pair of electrons is transferred from lactate to fumarate:V.a. The net potential (AE) of this reaction (expressed in 2 decimal places) isb. The standard Gibbs free energy change (AG) for this reaction (expressed in 3 significant figures; follow the format below) isJ/mol.c. The equilibrium constant (Kea) for this reaction (expressed in 3 significant figures) is

1) Oxidation is loss of electrons and reduction is gain of electrons. Oxidizing agent is a species…

Answered: Given the following standard reduction…

Chemical Principles in the Laboratory

11th Edition

ISBN:9781305264434

Author:Emil Slowinski, Wayne C. Wolsey, Robert Rossi

Publisher:Emil Slowinski, Wayne C. Wolsey, Robert Rossi

Chapter32: Voltaic Cell Measurements

Section: Chapter Questions

Problem 2ASA

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Halide ions can he deposited at a silver anode, the reaction being Ag(s) + X- AgX(s) +e- Suppose that a cell was formed by immersing a silver anode in an analyte solution that was 0.0250 M Cl-,Br-, and I -ions and connecting the half-cell to a saturated calomel cathode via a salt bridge. (a) Which halide would form first and at what potential? Is the cell galvanic or electrolytic? (b) Could I- and Br- be separated quantitatively? (Take 1.00 l0-5 M as the criterion for quantitative removal of an ion.) If a separation is feasible, what range of cell potential could he used? (c) Repeat part (b) for I- and Cl-. (d) Repeat part (b) for Br- and Cl-.
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.
2.( J Given the standard reduction potentials (E°) for ubiquinone (Q) and NADP+ provided below, consider the following questions. Q+ 2H+ + 2e ---> QH₂ NADP+ + H+ + 2e---> NADPH Eº⁹ = 0.04 V Eº⁹ = -0.32 V (a) ( Calculate the standard AEº for the oxidation of NADPH by Q. From the reactants in your derived redox reaction, indicate the oxidant and reductant. (b): .) Calculate the standard free energy of the redox reaction in part (a) and indicate if the reaction is exergonic or endergonic.
The reaction glyceraldehyde-3-phosphate NAD + P→ 1.3 diphosphoglycerate NADH+H has a standard reaction free energy (pH 7) of A.G 6.3 kJ mol ngchemistry.com/peycenView/assic Soffset-prev Part A If the standard reduction potential of NAD +H+2e →NADH is 0.324 V, the reaction 1,3 dphosphoglycerate+ADP 3-phosphoglyce+ATP has a standard reaction free energy (pH 7) of A,G= -18.8 kJ/mol and the ATP hydrolysis reaction ATP H20 ADP PH has a standard reaction free energy (pH 7) af-31.0 Kmo, cacutane the standard reduction polantial for the reaction phosphaglyser+2+31+ gyoeraldehyde-3-phosphate + H₂O Express your answer to three significant figures and include the appropriate units. Submi PA .574 Previous Ar V * Incorrect; Try Again; 3 attempts remaining Predous ten
Given the standard reduction potentials (Eo ’) for ubiquinone (Q) Q + 2H+ + 2e- ---> QH2 E o ’ = 0.04V FMN + 2H+ + 2e- ---> FMNH2 E o ’ = -0.22V Calculate the standard ΔEo ’ for the oxidation of FMNH2 by Q. Make sure to show each half reaction and the overall redox reaction. From the reactants in your derived redox reaction, indicate the oxidant and reductant
Kalan Süreniz: (Os 29d 34sn ) Ayn anda birden çok oturum açan kullanıcinın sınavi geçersiz sayılacaktir!. 1. 1) If a cell generates current by itself, that is, if it operates as a battery, the electrode marked (-) is the anode. II) E If an electric current is applied from outside, the electrode marked (-) is the anode. I) The electrode with a large oxidation potential in a Galvanic cell is marked (-). IV) In order for the battery to generate current by itself, the potential of the battery (Epil) must be positive. Which of the above is/are wrong. I ve III A-) Il ve II B-) I ve IV C-) Yalnızi D-) Yalnz IV E-) 19Bop hrat SORU3 O O O OO
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.
3. Consider the following coupled reaction: Isocitrate + NAD+ à à a-Ketoglutarate + CO2 + NADH First write the two standard half reactions written in reduction form for each with their std half reaction reduction potentials. Next calculate the AEo' for the reaction written above. Finally, based on the calculation convert this to the AGO
Given the standard reduction potentials (Eo ’) for ubiquinone (Q) Q + 2H+ + 2e- ---> QH2 E o ’ = 0.04 V FMN + 2H+ + 2e- ---> FMNH2 E o ’ = -0.22 V Calculate the standard ΔEo ’ for the oxidation of FMNH2 by Q. From the reactants in your derived redox reaction, indicate the oxidant and reductant. Then calculate the standard free energy of the redox reaction and indicate if the reaction is exergonic or endergonic.
calculate Delta G for the following reaction: Succinate + FAD -> Fumarate + FADH2 The standard reduction electric potentials of half-cell reactions are: FAD + 2H+ +2e- -> FADH2 Eo' = +0.05 V Fumarate + 2H+ + 2e- -> Succinate Eo' = +0.03 V Show your work (Refer to F = 96.5 kJ V-1 mol-1)
Calculate the standard free energy change (AG") for the transfer of electrons from succinate to ubiquinone: Succinate + ubiquinone O -2.7 kJ/mol relevant half-reactions and standard reduction potentials: fumarate + 2H* + 2 e™ H succinate ubiquinone + 2 H+ + 2 e² = O2.7 kJ/mol -8.7 kJ/mol O 14.7 kJ/mol succinate dehydrogenase O -6.0 kJ/mol Fumarate + ubiquinol ubiquinol E = 0.031 V ED - 0.045 V Atte 1 H
Q1. A Daniell Cell, the copper and zinc electrodes are immersed in a solution of 0.01M copper sulfateand 1 M zinc sulfate, respectively. What is the calculated cell potential E (V) for this cell?A. 1.10;B. 1.04;C. 1.05;D. 1.11;E. 1.14

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