Electron acceptor electron donor E' (mV) So+ 10H+ 8e HS + 4H,0 -220 NO+2H + 2e - NO, + H,0 +420 Use the table of reduction potentials to answer the question. Could a bacterium obtain energy using nitrite (NO,) as an electron donor and sulfate (SO,2) as a terminal electron accentor2 A) O Yes B) O No C) O Cannot be determined from the information given

Electron acceptor electron donor E' (mV) So+ 10H+ 8e HS + 4H,0 -220 NO+2H + 2e - NO, + H,0 +420 Use the table of reduction potentials to answer the question. Could a bacterium obtain energy using nitrite (NO,) as an electron donor and sulfate (SO,2) as a terminal electron accentor2 A) O Yes B) O No C) O Cannot be determined from the information given

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

Calculate the cell potential, E, for the given reactions at 25.00 "C using the ion concentrations provided. Then, determine if th cells are spontaneous or nonspontaneous as written. Refer to the table of standard reduction potentials (E). Pt(s) + Fe²(aq) = P² (aq) + Fe(s) [Fe²*1 = 0.0064 M E= incorrect -4761 E= Cu(s) + 2 Ag* (aq) = Cu² (aq) + 2 Ag(s) |Cu²+1 = 0.027 M Ag1=0.027 M E [P1²*1 = 0.067 M Co² (aq) + Ti (aq) — Co¹ (aq) + Ti² '(aq) Co²1 = 0.055 M Co= 0.030 M ITP 1 = 0.0070 M T² = 0.0107 M mam V The cell is not spontaneous spontaneous. The cell is spontaneous not spontaneous. incorrect The cell is spontaneous not spontaneoux.
Calculate the concentration of an unknown solution in a concentration cell. A concentration cell consisting of two hydrogen electrodes (P H2- latm), where the cathode is a standard hydrogen electrode and the anode solution has an unknown pH, has a cell voltage of 0.193 V. What is the pH in the unknown solution? Assume the temperature of the solutions is 298 K. !! pH =
Consider the following standard reduction potentials in acid solution: E°(V) Al⁺³ + 3e− → Al(s) −1.66 Ag⁺¹ + e− → Ag(s) +0.80 Sn⁺⁴ + 2e− → Sn⁺² +0.14 Fe⁺³ + e− → Fe⁺² +0.77 The strongest reducing agent among those shown above is A) Al⁰ B) Fe⁺³ C) Br⁻ D) Al⁺³
3q112 please answer with solutions thanks
29b
Standard Reduction Potentials at 25 °C Half-reaction. Eº(volts) Au³+ + 2e Au+ 1.290 Aut+eAu 1.680 Au³+ + 3e →→Au 1.420 In a disproportionation reaction, the same species is oxidized and reduced. Use the data given above to analyze the disproportionation reaction: 3Aut 2Au + Au³+ Will Au* disproportionate in aqueous solution? To justify your answer, what is the standard cell voltage for the disproportionation reaction?
Help with the following question
1. Consider the following standard reduction potentials in acid solution: E°(V) -1.66 +0.07 +0.14 Fe³+ + e +0.77 The strongest reducing agent among those shown above is Hint: If answer is with charge, type this way: X2+ Al³+ + 3e → Al(s) AgBr(s) + e → Ag(s) + Brā Sn4+ + 2e → + 2e → Sn²+ Fe²+
Consider the following standard reduction potentials: F2(g) + 2 e - 2 F (aq) E° = +2.87 V Mg2*(aq) + 2 e - Mg(s) E° = -2.37 V Under standard conditions, O Mg(s) is a stronger oxidizing agent than F (aq), and Mg2*(aq) is a stronger reducing agent than F2(g), O F (aq) is a stronger oxidizing agent than Mg(s), and F2(g) is a stronger reducing agent than Mg2*(aq). O F2(g) is a stronger oxidizing agent than Mg-"(aq), and Mg(s) is a stronger reducing agent than F (aq). O Mg2*(aq) is a stronger oxidizing agent than F2(g), and F(aq) is a stronger reducing agent than Mg(s).
Use the standard reduction potentials located in the "Tables' linked above to calculate the standard free energy change in kJ for the reaction: 3Hg"(aq) + 2Cr(s)3Hg(1) + 2Cr*(aq) Answer: |kJ K for this reaction would be than one.
Enter electrons as e". Use smallest possible integer coefficients. States are not required. If a box is not needed, leave it blank. Standard Reduction Potentials (Volts) at 25 °C Cl₂ (g) + 2 e →2 Cl(aq) O2(g) + 4 H3O+ (aq) + 4 e 6 H₂O(1) 1.360 1.229 2 H2O(l) + 2e Al3+ (aq) + 3 e → Al (s) H2(g) + 2 OH(aq) -0.828 -1.660 A 0.114 M neutral aqueous AlCl3 solution is electrolyzed under 1 atm pressure using platinum electrodes. (a) Write the half-reactions expected to occur, taking into account the effect of the non-standard conditions on the electrode potentials. Half-reaction at anode: + + + + Half-reaction at cathode: + + + + (b) What is the expected decomposition potential?
Shown below are some standard reduction potentials. For which of these compounds is oxidation most favorable? (Imagine you mixed all four of these compounds together in equal quantities. Which one would get oxidized?) a) H2O b) NADH c) O2 d) NAD+