32Below are the paired reduction reactions for chemolithotrophic denitrification: these organisms are using nitrate as an electron accepter and are using hydrogen gas as a sourceof energy and electrons.2NO+10e-> N₂ (+0.74 volts)•2H+2e-> H₂ (-0.42 volts)Using the information given, calculate the AE for this reaction, balance the full reaction to determinen, the number of electrons transfered when 130 moles of Hy are cxidized.Finally, use the simplified Nernst EquationAG--nFAE, where F-96.5 kJ (ex V¹to determine the Gibbs Free energy available to do work!• Report your answer in kJ in standard decimal notation rounded to two decimal placesIncluding trailing zeros, even if it is a whole numbereg. 18.00, not 18.Report only the numeric portion of your answereg 101. not 1.01 kj per mole• Answers should ALWAYS be negative since this is a spontaneous reaction.-14.552.2

We have to find the value of standard reduction potential.

Below are the paired reduction reactions for chemolithotrophic denitrification: these organisms are using nitrate as an electron accepter and are using hydrogen gas as a source of energy and electrons. 2NO+10e->N₂ (+0.74 volts) 2H+2H₂ (-0.42 volts) Using the information given, calculate the AE for this reaction, balance the full reaction to determinen, the number of electrons transfered when 130 moles of H₂ are oxidized. Finally, use the simplified Nernst Equation AG--FAE, where F-96.5 Kle=V¹ to determine the Gibbs Free energy available to do work! • Report your answer in kJ in standard decimal notation rounded to two decimal places. Including trailing zeros, even if it is a whole number eg 18.00, not 18 Report only the numeric portion of your answer eg 101.not 1.01 kj per mole Answers should ALWAYS be negative since this is a spontaneous reaction. -14.552.2

Below are the paired reduction reactions for chemolithotrophic denitrification: these organisms are using nitrate as an electron accepter and are using hydrogen gas as a source of energy and electrons. 2NO+10e->N₂ (+0.74 volts) 2H+2H₂ (-0.42 volts) Using the information given, calculate the AE for this reaction, balance the full reaction to determinen, the number of electrons transfered when 130 moles of H₂ are oxidized. Finally, use the simplified Nernst Equation AG--FAE, where F-96.5 Kle=V¹ to determine the Gibbs Free energy available to do work! • Report your answer in kJ in standard decimal notation rounded to two decimal places. Including trailing zeros, even if it is a whole number eg 18.00, not 18 Report only the numeric portion of your answer eg 101.not 1.01 kj per mole Answers should ALWAYS be negative since this is a spontaneous reaction. -14.552.2

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

Consider a modification to the Hall-Heroult process for aluminum production, where we keep things the same but replace the carbon electrode by something inert. The original process requires three electrons to produce one atom of Al metal and is: (1/2) Al½O3 + (3/4) C → Al + (3/4) CO2 Suppose that the new process also requires three electrons and is (1/2) Al,O; → Al + (3/4) O2 If the energy, E, produced from the reaction C + O2 → CO2 is 4.08 eV per carbon atom, how much would the voltage need to be increased in order produce aluminum assuming that the energy from the oxidation of carbon to carbon dioxide is replaced by electrical energy in the process?
Table 20.1 Half Reaction F2 (g) + 2e7 Cl2 (g) + 2e Br2 (1) + 2e 2C1™ (aq) 2Br (aq) O2 (g) + 4H+ (aq) + 4e¯ Ag (s) → Ag+ e Fe3+ (aq) + e 12 (s) + 2e™ Cu2+ + 2e 2H+ 2e Pb2+ + 2e™ Ni2+ + 2e Lit + e 2F (aq) - Fe2+ (aq) 21 (aq) Cu (s) H2 (8) Pb (s) Ni (s) Li (s) E°(V) +2.87 +1.359 +1.065 2H₂0 (1) +1.23 +0.799 +0.771 +0.536 +0.34 0 -0.126 -0.28 -3.05 21) Using Table 20.1, which substance can oxidize I (aq) to 12 (s)? A) Cu²+ (aq) B) Br (aq) C) Ag (s) D) Br2 (1) E) Ni2+ (aq)
19.39
How many grams of X (MW = 44.20 g/mol)(in g) will be deposited on a cathode in 1.91 h by a current of 3.8 A? X4+ + 4e- → X(s)
In the Hall - Heroult process, aluminum is produced by the electrolysis of molten Al₂O3(0). The half reactions are C(s) +20²- (aq) → CO₂(g) + 4e¯ Al³+ +3e → Al(s) (aq) The mass of Al(s) produced for 2.00 kg of C(s) consumed is (round to the nearest kg) 6.00 kg 1.69 kg 2.45 kg 3.00 kg
In Electrochemical cells electrons are transfered from the reactants being reduced to the reactants being oxidized through a wire connecting the two containers. (True/False)
Balance the following equation in basic solution: CN- + Mn0,¯- CNO- + Mn02 What type of electrode material is use to construct bacterial fuel cells in order for the bacteria grow naturally on the surface of electrodes? Discuss the advantages and disadvantages of fuel cells over conventional power plants in producing electricity.
19.37
In the following reaction, identify the reactant that is oxidized and the reactant that is reduced: 2FeO(s) → 2Fe(s) + O2(g) Half-equations: for Fe2+ in FeO: 2Fe2+ + 4e–→ 2Fe for O2– in FeO: 2O2–→ O2 + 4e– A. Fe2+ in FeO is reduced, while O2– in FeO is oxidized. B. Fe2+ in FeO is oxidized, while O2– in FeO is reduced. C. Both Fe2+ and O2– in FeO are oxidized. D. Both Fe2+ and O2– in FeO are reduced.
A battery relies on the oxidation of magnesium and the reduction of Cu2+. The initial concentrations of Mg2+ and Cu2+ are 1.0x104 mol/L and 1.5 mol/L, respectively, in 1.0-litre half- cells. How long can the battery deliver 4 A before going dead? Express your answer in hours using two significant figures.
Use standard reduction potentials to calculate the standard free energy change in kJ for the reaction: 2H+ (aq) + Hg(1)→ H₂(g) + Hg²+ (aq) 2H+ (aq) + 2e¯ → H₂(g) Fº red 2+ Hg2 (aq) + 2e¯ → Hg(1) AGO = || kJ K for this reaction would be Eº red = 0.000 V = = 0.855 V than one.
OCHEM HELP!!! Provide ALL the resonance structures for the compounds shown below (see the attached picture). Also draw ALL the valence electrons (lone pairs) on the given compound and the resonance structures drawn and use the correct arrows between the resonance structures drawn