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+ (+0.34 volts) • O₂ +4e-> 2H₂O (+0.82 volts) Using the information given, calculate the AE for this reaction, balance the full reaction to determine the n, the number of electrons transferred when 30 moles of NH4* are oxidized. Finally, use the simplified Nernst Equation AG = -nFAE, where F = 96.5 kJ (mol e x V)-¹ to determine the Gibbs Free energy available to do work! • Report your answer in kJ rounded to two decimal places. o Include trailing zeros!! Always report two decimal places even if the answer is a whole number o e.g. 18.00 not 18 • Report only the numeric portion of your answer o e.g. 1.01, not 1.01 kj per mole. • Answers should ALWAYS be negative since this is a spontaneous reaction. Type your answer

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+ (+0.34 volts) • O₂ +4e-> 2H₂O (+0.82 volts) Using the information given, calculate the AE for this reaction, balance the full reaction to determine the n, the number of electrons transferred when 30 moles of NH4* are oxidized. Finally, use the simplified Nernst Equation AG = -nFAE, where F = 96.5 kJ (mol e x V)-¹ to determine the Gibbs Free energy available to do work! • Report your answer in kJ rounded to two decimal places. o Include trailing zeros!! Always report two decimal places even if the answer is a whole number o e.g. 18.00 not 18 • Report only the numeric portion of your answer o e.g. 1.01, not 1.01 kj per mole. • Answers should ALWAYS be negative since this is a spontaneous reaction. Type your 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

Calculate the standard free energy change in kJ given the standard reduction potentials for the half reactions of the following hypothetical elements: X3+(aq) + e- → X2+(aq) SRP: +0.7 V Y2(ℓ) + 2e- → 2Y-(aq) SRP: +0.35 V
Sa+4 is the strongest oxidizing of 7) Calculate the equilibrium constant for the reaction at 25°C. 3 Zn(s) + 2 Fe³(aq) = 3 Zn¹²(aq) + 2 Fe(s)
Answer the four questions below related to the spontaneous redox reaction that occurs whenCr(OH)3(s) reacts with NO3–(aq) to produce CrO42–(aq)and NO2–(aq) under basic conditions. Write the balanced net ionic equation, including states of matter, for the overall reaction.
In the following half reaction, what class of reaction is shown? 202 (aq) 0₂ (8) + 4e dissociation decomposition oxidation. O replacement O reduction
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
Based on the following electrochemical data, which is the strongest oxidizing agent? Hg2+(aq) + 2e → Hg(1) E°red = +0.85 V Cr20-2 (aq) + 14H*(aq) + 6e¨ → 2Cr³+(aq) + 7H2O(1I) E°red = +1.33 V Ca2+(aq) + 2e → Ca(s) E°red = -2.76 V Zn2+(aq) + 2e → Zn(s) E°red = -0.76 V %3D NO3 (aq) + 4H*(aq) + 3e¯ → NO(g) + 2H2O(1) E°red = +0.96 V O A) Zn2+ B) Zn(s) C) Cr20-²- D) Ca2+ E) NO3 F) Ca(s)
Write a balanced half-reaction for the reduction of CrO 4 2–(aq) to Cr(OH) 3(s) in a basic solution.
Calculate the standard free energy change in kJ given the standard reduction potentials for the half reactions of the following hypothetical elements: X3+(aq) + e- → X2+(aq) SRP: -0.64 V Y2(ℓ) + 2e- → 2Y-(aq) SRP: -0.34 V
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.
Calculate the equilibrium constant for the following reactions at 25°C from reduction potential data: (a) Cu2+(aq) + Cu(s) ⇌ 2Cu+(aq)
Calculate the standard free energy change in kJ given the standard reduction potentials for the half reactions of the following hypothetical elements: X3+(aq) + e- → X2+(aq) SRP: -0.69 V Y2(ℓ) + 2e- → 2Y-(aq) SRP: -0.44 V
Chromium can be electroplated from aqueous potassium dichromate, with the reduction shown below: Cr20,2- (aq) (ag) + 12e → 2Cr(s) + 7H20 How many moles of electrons can be generated from 200 mL of 1.94 M K2C1207?